Chemistry 12th Edition By Chang – Test Bank

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Chemistry 12th Edition By Chang – Test Bank

Chapter 06

Thermochemistry

 

 

Multiple Choice Questions

Radiant energy is

  1. the energy stored within the structural units of chemical substances.
    B. the energy associated with the random motion of atoms and molecules.
    C. solar energy, i.e. energy that comes from the sun.
    D. energy available by virtue of an object’s position.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.01
Subtopic: Units of Energy
Topic: Thermochemistry

  1. Thermal energy is 4
    A.the energy stored within the structural units of chemical substances.
    B. the energy associated with the random motion of atoms and molecules.
    C. solar energy, i.e. energy that comes from the sun.
    D. energy available by virtue of an object’s position.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.01
Subtopic: Units of Energy
Topic: Thermochemistry

 

 

 

 

  1. Chemical energy is
    A.the energy stored within the structural units of chemical substances.
    B. the energy associated with the random motion of atoms and molecules.
    C. solar energy, i.e. energy that comes from the sun.
    D. energy available by virtue of an object’s position.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.01
Subtopic: Units of Energy
Topic: Thermochemistry

  1. Potential energy is
    A.the energy stored within the structural units of chemical substances.
    B. the energy associated with the random motion of atoms and molecules.
    C. solar energy, i.e. energy that comes from the sun.
    D. energy available by virtue of an object’s position.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.01
Subtopic: Units of Energy
Topic: Thermochemistry

  1. Heat is
    A.a measure of temperature.
    B. a measure of the change in temperature.
    C. a measure of thermal energy.
    D. a measure of thermal energy transferred between two bodies at different temperature.

 

Bloom’s Level: 2. Understand
Difficulty: Medium
Gradable: automatic
Section: 06.02
Subtopic: System/Surroundings and Heat/work
Subtopic: Units of Energy
Topic: Thermochemistry

 

 

 

 

  1. An endothermic reaction causes the surroundings to
    A.warm up.
    B. decrease in temperature.
    C. become acidic.
    D. release CO2.
    E. condense.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.02
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. An exothermic reaction causes the surroundings to
    A.increase in temperature
    B. decrease in temperature.
    C. become acidic.
    D. release CO2.
    E. expand.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.02
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. Aluminum metal has a specific heat of 0.900 J/g·°C. Calculate the amount of heat required to raise the temperature of 10.5 moles of Al from 30.5 °C to 225°C.
    A.1.84 kJ
    B. 2.41 kJ
    C. 65.1 kJ
    D. 49.6 kJ
    E. 57.3 kJ

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. Given the specific heat for aluminum is 0.900 J/g·°C, how much heat is released when a 3.8 g sample of Al cools from 450.0°C to 25°C?
    A.54 J
    B. 60 J
    C. 86 J
    D. 1.5 kJ
    E. 1.7 kJ

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. Calculate the amount of heat necessary to raise the temperature of 135.0 g of water from 50.4°F to 85.0°F. The specific heat of water = 4.184 J/g·°C.
    A.1.1 kJ
    B. 10.9 kJ
    C. 16.6 kJ
    D. 19.5 kJ
    E. 48.0 kJ

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. How much heat is required to raise the temperature of 1.5 x 103 g of water from 45°F to 130.°F? The specific heat of water is 4.184 J/g·°C.
    A.3.0 x 101 kJ
    B. 3.0 x 102 kJ
    C. 3.4 x 102 kJ
    D. 5.3 x 102 kJ
    E. 8.2 x 102 kJ

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. Three separate 3.5g blocks of Al, Cu, and Fe at 25°C each absorb 0.505 kJ of heat. Which block reaches the highest temperature? The specific heats of Al, Cu, and Fe are 0.900 J/g·°C, 0.385J/g·°C, and 0.444 J/g·°C, respectively.
    A.Al
    B. Cu
    C. Fe
    D. Al and Cu
    E. Fe and Cu

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. A beaker contains 115 g of ethanol at 18.2°C. If the ethanol absorbs 1125 J of heat without losing heat to the surroundings, what will be the final temperature of the ethanol? The specific heat of ethanol is 2.46 J/g´°C.
    A.4.08°C
    B. 14.1°C
    C. 18.4°C
    D. 22.2°C
    E. 36.4°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. A 22.0 g block of copper at 45°C absorbs 2.50 kJ of heat. Given the specific heat of Cu is 0.385 J/g·°C what will be the final temperature of the Cu?
    A.45°C
    B. 340.°C
    C. 295°C
    D. 30.°C
    E. 250.°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. If 10.6 moles of water at 35°C absorbs 12.30 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g·°C.
    A.15°C
    B. 20°C
    C. 35°C
    D. 50.°C
    E. 312°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. A 135 g sample of H2O at 85°C is cooled. The water loses a total of 15 kJ of energy in the cooling process. What is the final temperature of the water? The specific heat of water is 4.184 J/g·°C.
    A.27°C
    B. 58°C
    C. 70°C
    D. 84°C
    E. 112°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper?
    A.0.385 J/g·°C
    B. 1.32 J/g·°C
    C. 2.60 J/g·°C
    D. 24.5 J/g·°C
    E. 1.83 ´ 104 J/g·°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. The specific heat of gold is 0.129 J/g·°C. What is the molar heat capacity of gold?
    A.0.039 J/mol·°C
    B. 0.129 J/mol·°C
    C. 25.4 J/mol·°C
    D. 39.0 kJ/mol·°C
    E. 197 J/mol·°C

 

Bloom’s Level: 3. Apply
Difficulty: Easy
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. Suppose a 50.0 g block of silver (specific heat = 0.2350 J/g·°C) at 100°C is placed in contact with a 50.0 g block of iron (specific heat = 0.4494 J/g·°C) at 0°C, and the two blocks are insulated from the rest of the universe. The final temperature of the two blocks
    A.will be higher than 50°C.
    B. will be lower than 50°C.
    C. will be exactly 50°C.
    D. is unrelated to the composition of the blocks.
    E. cannot be predicted.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is –26.42 kJ/g.
    A.1.34 kJ/°C
    B. 4.18 kJ/°C
    C. 5.52 kJ/°C
    D. 15.87 kJ/°C
    E. 752.1 kJ/°C

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. The heat of combustion of naphthalene is –40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of 4.21°C was observed. What is the heat capacity of the bomb calorimeter excluding the water?
    A.1.76 kJ/°C
    B. 3.64 kJ/°C
    C. 7.8 kJ/°C
    D. 15.3 kJ/°C
    E. 32.9 kJ/°

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: First Law of Thermodynamics
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. Which of the following processes is exothermic?
    A.CH4(g) + 2 O2(g) ® CO2(g) + 2 H2O(l)
    B. CO2(g) + 2 H2O(l) ® CH4(g) + 2 O2(g)
    C. CO2(s) ®CO2(g)
    D. H2O(l) ®H2O(g)
    E. 6 H2O(g) + 4 CO2(g) ® 2 C2H6(g) + 7 O2(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.02
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

Which of the following processes is exothermic, given the following:
N2(g) + 2 O2(g) ® N2O4(l) DH° = 9.67 kJ/mol
N2(g) + 2 O2(g) ® 2 NO2(g) DH° = 67.70 kJ/mol

  1. 2 N2(g) + 4 O2(g) ® 2 N2O4(l)
    B. ½ N2(g) + O2(g) ® ½ N2O4(l)
    C. N2O4(l) ®N2(g) + 2 O2(g)
    D. 2 N2(g) + 4 O2(g) ® 2 NO2(g) + N2O4(l)
    E. 2 N2(g) + 4 O2(g) ® 4 NO2(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

 

Which of the following processes is endothermic, given the following:
S(s) + O2(g) ®SO2(g) DH = –299 kJ/mol
S(s) + 3/2 O2(g) ®SO3(g) DH = –395 kJ/mol

  1. 2 S(s) + 2 O2(g) ®2 SO2(g)
    B. ½ S(s) + ½ O2(g) ®½ SO2(g)
    C. 2 S(s) + 5/2 O2(g) ® SO2(g) + SO3(g)
    D. SO3(g) ®S(s) + 3/2 O2(g)
    E. 2 S(s) + 3 O2(g) ®2 SO3(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

  1. Which of the following processes is endothermic?
    A.O2(g) + 2H2(g) ® 2H2O(g)
    B. H2O(g) ®H2O(l)
    C. 3O2(g) + 2CH3OH(g) ® 2CO2(g) + 2H2O(g)
    D. H2O(s) ®H2O(l)

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.04
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

 

A 100. mL sample of 0.200 M aqueous hydrochloric acid is added to 100. mL of 0.200 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water) is 480. J/K. The following reaction occurs when the two solutions are mixed.
HCl(aq) + NH3(aq) ®NH4Cl(aq)
The temperature increase is 2.34°C. Calculate DH per mole of HCl and NH3 reacted.

  1. –154 kJ/mol
    B. –1.96 kJ/mol
    C. 1.96 kJ/mol
    D. 154 kJ/mol
    E. 485 kJ/mol

 

Bloom’s Level: 5. Evaluate
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

  1. A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium.
    Mg(s) + 1/2O2(g) ®MgO(s)
    A.–3280 kJ/mol
    B. –602 kJ/mol
    C. –24.8 kJ/mol
    D. 106 kJ/mol
    E. 435 kJ/mol

 

Bloom’s Level: 5. Evaluate
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

  1. The reaction that represents the standard enthalpy of formation for acetone (CH3COCH3), a common ingredient in nail polish remover is:
    A.3 C(graphite) + 3 H2(g) + ½ O2(g) ® CH3COCH3(l)
    B. 6 C(diamond) + 6 H2(g) + O2(g) ® 2 CH3COCH3(l)
    C. 3 C(diamond) + 3 H2(g) + ½ O2(g) ® CH3COCH3(l)
    D. CH3COCH3(l) ®3 C(graphite) + 3 H2(g) + ½ O2(g)
    E. CH3COCH3(l) + 4 O2(g) ® 3 CO2(g) + 3 H2O(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

  1. The reaction that represents the standard enthalpy of formation for sucrose (C12H22O11) is:
    A.C12H22O11(s) + 12 O2 ® 12 CO2(g) + 11 H2O(g)
    B. 12 C(diamond) + 11 H2(g) + 11/2 O2(g) ® C12H22O11(s)
    C. 12 C(graphite) + 11 H2(g) + 11/2 O2(g) ®C12H22O11(s)
    D. 24 C(diamond) + 22 H2(g) + 11 O2(g) ® 2 C12H22O11(s)
    E. C12H22O11(s) ®12 C(graphite) + 11 H2(g) + 11/2 O2(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

  1. The reaction that represents the standard enthalpy of formation for benzene (C6H6) is:
    A.6 C(diamond) + 3 H2(g) ® C6H6(l)
    B. 6 C(graphite) + 6 H(g) ® C6H6(l)
    C. C6H6(l) + 15/2 O2(g) ® 6 CO2(g) + 3 H2O(g)
    D. 6 C(graphite) + 3 H2(g) ® C6H6(l)
    E. C6H6(l) ®6 C(graphite) + 3 H2(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Which of the following has a DH°f= 0 kJ/mol?

  1. CO2(g)
    B. O3(g)
    C. Cl(aq)
    D. NH3(aq)
    E. I2(s)

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Which of the following has a DH°f= 0 kJ/mol?

  1. NO(g)
    B. CS2(l)
    C. Fe2+(aq)
    D. H2O(l)
    E. N2(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Easy
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

When 0.560 g of Na(s) reacts with excess F2(g) to form NaF(s), 13.8 kJ of heat is evolved at standard-state conditions. What is the standard enthalpy of formation (DH°f) of NaF(s)?

  1. -570 kJ/mol
    B. –24.8 kJ/mol
    C. –7.8 kJ/mol
    D. 24.8 kJ/mol
    E. 570 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at standard-state conditions. What is the standard enthalpy of formation (DH°f) of HgO(s)?

  1. –90.7 kJ/mol
    B. –7.75 kJ/mol
    C. 0.419 kJ/mol
    D. 27.9 kJ/mol
    E. 143 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Ethanol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. The standard heat of combustion of ethanol, C2H5OH(l), is –1366.8 kJ/mol. Given that DH°f[CO2(g)] = –393.5 kJ/mol and DH°f[H2O(l)] = –285.8 kJ/mol, what is the standard enthalpy of formation of ethanol?

  1. –687.6 kJ/mol
    B. –277.6 kJ/mol
    C. 687.6 kJ/mol
    D. 1,367 kJ/mol
    E. 3,010 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: heat of combustion of C2H4(g)= –1411 kJ/mol; DH°f[CO2(g)] = –393.5 kJ/mol; DH°f[H2O(l)] = –285.8 kJ/mol.

  1. 52 kJ/mol
    B. 87 kJ/mol
    C. 731 kJ/mol
    D. 1.41 ´ 103 kJ/mol
    E. 2.77 ´ 103 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Octane (C8H18) undergoes combustion according to the following thermochemical equation:
2C8H18(l) + 25O2(g) ® 16CO2(g) + 18H2O(l), DH°rxn = –11,020 kJ/mol.
Given that DH°f[CO2(g)] = –393.5 kJ/mol and DH°f[H2O(l)] = –285.8 kJ/mol, calculate the standard enthalpy of formation of octane.

  1. –210 kJ/mol
    B. –11,230 kJ/mol
    C. 22,040 kJ/mol
    D. –420 kJ/mol
    E. 420 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Acetylene (C2H2) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given DH°f[CO2(g)] = –393.5 kJ/mol, DH°f[H2O(g)] = –241.8 kJ/mol, and DH°f[C2H2(g)] = 226.6 kJ/mol, how much energy is released (kJ) when 10.5 moles of acetylene is burned?

  1. 2,510.8 kJ
    B. 26,400 kJ
    C. 13,200 kJ
    D. 52,700 kJ
    E. 9,050 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Butane (C4H10) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given DH°f[C4H10(g)] = –124.7 kJ/mol, DH°f[CO2(g)] = –393.5 kJ/mol, DH°f[H2O(g)] = –241.8 kJ/mol, how much energy is released (kJ) when 8.30 g of butane is burned?

  1. 22,100 kJ
    B. 2,658.3 kJ
    C. 379 kJ
    D. 759 kJ
    E. 2,910 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is given by the equation
4C2H5O2N(s) + 9O2(g) ® 8CO2(g) + 10H2O(l) + 2N2(g) DH°rxn = –3857 kJ/mol
Given that DH°f[CO2(g)] = –393.5 kJ/mol and DH°f[H2O(l)] = –285.8 kJ/mol, calculate the enthalpy of formation of glycine.

  1. –3,178 kJ/mol
    B. –964 kJ/mol
    C. –537.2 kJ/mol
    D. –268.2 kJ/mol
    E. 2,149 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Styrene, C8H8, is one of the substances used in the production of synthetic rubber. When styrene burns in oxygen to form carbon dioxide and liquid water under standard-state conditions at 25°C, 42.62 kJ are released per gram of styrene. Find the standard enthalpy of formation of styrene at 25°C.
(Given: DH°f[CO2(g)] = –393.5 kJ/mol, DH°f[H2O(l)] = –285.8 kJ/mol, DH°f[H2O(g)] = –241.8 kJ/mol)

  1. 147.8 kJ/mol
    B. 323.8 kJ/mol
    C. ~636.7 kJ/mol
    D. ~4249 kJ/mol
    E. ~8730 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Given 2Al(s) + (3/2)O2(g) ® Al2O3(s), DH°f = –1,670 kJ/mol for Al2O3 (s).
Determine DH° for the reaction 2Al2O3(s) ®4Al(s) + 3O2(g).

  1. –3,340 kJ/mol
    B. –1,670 kJ/mol
    C. –835 kJ/mol
    D. 1,670 kJ/mol
    E. 3,340 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Calculate the standard enthalpy of formation of liquid methanol, CH3OH(l), using the following information:

  1. –1,691.5 kJ/mol
    B. –238.7 kJ/mol
    C. –47.1 kJ/mol
    D. 47.1 kJ/mol
    E. 1691.5 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Calculate the standard enthalpy change for the reaction
2C8H18(l) + 17O2(g) ® 16CO(g) + 18H2O(l).
Given

  1. –10.450 kJ/mol
    B. –6,492 kJ/mol
    C. 6,492 kJ/mol
    D. 10,450 kJ/mol
    E. 15,550 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

During volcanic eruptions, hydrogen sulfide gas is given off and oxidized by air according to the following chemical equation:
2H2S(g) + 3O2(g) ® 2SO2(g) + 2H2O(g)
Calculate the standard enthalpy change for the above reaction given:

  1. –1036.1 kJ/mol
    B. –742.3 kJ/mol
    C. –149.5 kJ/mol
    D. 443.3 kJ/mol
    E. 742.3 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Calculate the standard enthalpy change for the reaction
2C8H18(l) + 21O2(g) ® 8CO(g) + 8CO2(g) + 18H2O(l).
Given:
2C8H18(l) + 25O2(g) ® 16CO2(g) + 18H2O(l) DH° = –11,020 kJ/mol
2CO(g) + O2(g) ® 2CO2(g) DH° = –566.0 kJ/mol

  1. –1.0454 ´ 104 kJ/mol
    B. –8,756 kJ/mol
    C. –6,492 kJ/mol
    D. 1.0454 ´ 104 kJ/mol
    E. 1.1586 ´ 104 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Calculate the standard enthalpy change for the reaction
2A + 2A2 + 4AB + B ® 5A2B
Given:

  1. – 95.0 kJ/mol
    B. – 60.0 kJ/mol
    C. – 15.0 kJ/mol
    D. 10.0 kJ/mol
    E. 45.0 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

Calculate the standard enthalpy change for the reaction
4A + 2B ® 2AB + A2
Given:

  1. – 95.0 kJ/mol
    B. – 60.0 kJ/mol
    C. – 15.0 kJ/mol
    D. 10.0 kJ/mol
    E. 45.0 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Calculate the heat required when 2.50 mol of A reacts with excess B and A2B according to the reaction:
2A + B + A2B ® 2AB + A2
Given:

  1. 10.0 kJ
    B. 12.5 kJ
    C. 25.0 kJ
    D. 35.0 kJ
    E. 62.5 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

How much heat (kJ) is evolved when 4.50 g of Fe2O3 is reacted with excess carbon monoxide using the equation below?
Fe2O3(s) + 3CO(g) ® 2 Fe(s) + 3 CO2(g) DH°rxn = – 24.8 kJ/mol,

  1. 0.699 kJ
    B. 2.10 kJ
    C. 17.9 kJ
    D. 24.8 kJ
    E. 112 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

 

Given H2(g) + (1/2)O2(g) ® H2O(l), DH° = –286 kJ/mol, determine the standard enthalpy change for the reaction 2H2O(l) ® 2H2(g) + O2(g).

DH° = –286 kJ/mol

DH° = +286 kJ/mol

DH° = –572 kJ/mol

DH° = +572 kJ/mol

DH° = –143 kJ/mol

 

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.06
Topic: Thermochemistry

 

 

 

Pentaborane B5H9(s) burns vigorously in O2 to give B2O3(s) and H2O(l). Calculate DHrxn for the combustion of 5.00 mol of B5H9.
DH°f[B2O3(s)] = –1,273.5 kJ/mol
DH°f[B5H9(s)] = 73.2 kJ/mol
DH°f[H2O(l)] = –285.8 kJ/mol

  1. – 45,400 kJ
    B. 45,400 kJ
    C. – 22,700 kJ
    D. – 9,090 kJ
    E. – 8,790 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

Concerning the reaction

how many grams of C(graphite) must be burned to release 275 kJ of heat?

  1. 0.70 g
    B. 8.40 g
    C. 12.0 g
    D. 17.1 g
    E. 22.3 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

The combustion of butane produces heat according to the equation
2C4H10(g) + 13O2(g) ® 8CO2(g) + 10H2O(l), DH°rxn= –5,314 kJ/mol.
How many grams of butane must be burned to release 1.00 ´ 104 kJ of heat?

  1. 30.9 g
    B. 61.8 g
    C. 109 g
    D. 153 g
    E. 219 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

The combustion of butane produces heat according to the equation
2C4H10(g) + 13O2(g) ® 8CO2(g) + 10H2O(l), DH°rxn= –5,314 kJ/mol.
How many grams of CO2 are produced per 1.00 ´ 104 kJ of heat released?

  1. 23.4 g
    B. 44.0 g
    C. 82.3 g
    D. 187 g
    E. 662 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

Given that CaO(s) + H2O(l) ® Ca(OH)2(s), DH°rxn = –64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?

  1. 6.92 g
    B. 56.1 g
    C. 455 g
    D. 606 g
    E. 3.40 ´ 104 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

The combustion of pentane produces heat according to the equation
C5H12(l) + 😯2(g) ® 5CO2(g) + 6H2O(l), DH°rxn= –3,510 kJ/mol.
How many grams of CO2 are produced per 2.50 ´ 103 kJ of heat released?

  1. 0.0809 g
    B. 3.56 g
    C. 31.3 g
    D. 157 g
    E. 309 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

An average home in Colorado requires 20. GJ of heat per month. How many grams of natural gas (methane) must be burned to supply this energy?
CH4(g) + 2O2(g) ® CO2(g) + 2H2O(l) DH°rxn= –890.4 kJ/mol

  1. 7.1 ´ 10–4 g
    B. 1.4 ´ 103 g
    C. 1.4 ´ 104 g
    D. 2.2 ´ 104 g
    E. 3.6 ´ 105 g

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

Given the thermochemical equation 2SO2(g) + O2(g) ® 2SO3(g), DH°rxn= –198 kJ/mol, how much heat is evolved when 600. g of SO2 is burned?

  1. 5.46 ´ 10–2 kJ
    B. 928 kJ
    C. 1.85 ´ 103 kJ
    D. 3.71 ´ 103 kJ
    E. 59,400 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

Determine the heat given off to the surroundings when 9.0 g of aluminum reacts according to the equation 2Al + Fe2O3 ® Al2O3 + 2Fe, DH°rxn= –849 kJ/mol.

  1. 1.4 ´ 102 kJ
    B. 2.8 ´ 102 kJ
    C. 5.6 ´ 102 kJ
    D. 2.5 ´ 103 kJ
    E. 7.6 ´ 103 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

Find the heat absorbed from the surroundings when 15 g of O2 reacts according to the equation O + O2 ® O3, DH°rxn= –103 kJ/mol.

  1. 4.6 ´ 10–3 kJ
    B. 32 kJ
    C. 48 kJ
    D. 96 kJ
    E. 110 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

Ethanol (C2H5OH) burns according to the equation
C2H5OH(l) + 3O2(g) ® 2CO2(g) + 3H2O(l), DH°rxn = –1367 kJ/mol.
How much heat is released when 35.0 g of ethanol is burned?

  1. 9.61 ´ 10–4 kJ
    B. 1,040 kJ
    C. 1,367 kJ
    D. 1,797 kJ
    E. 4.78 ´ 104 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

Methanol (CH3OH) burns according to the equation
2CH3OH(l) + 3O2(g) ® 2CO2(g) + 4H2O(l), DH°rxn = –1454 kJ/mol.
How much heat, in kilojoules, is given off when 75.0 g of methanol is burned?

  1. 727 kJ
    B. 3.22 ´ 103 kJ
    C. 1.45 ´ 103 kJ
    D. 1.70 ´ 103 kJ
    E. 3.41 ´ 103 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Topic: Thermochemistry

 

 

 

Calcium oxide and water react in an exothermic reaction:
CaO(s) + H2O(l) ® Ca(OH)2(s), DH°rxn = –64.8 kJ/mol.
How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152g H2O?

  1. 1.97 ´ 10–3 kJ
    B. 8.26 kJ
    C. 508 kJ
    D. 547 kJ
    E. 555 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Subtopic: Calorimetry (Measuring Heats of Reaction)
Topic: Thermochemistry

 

 

Solid sodium peroxide (Na2O2) reacts with liquid water yielding aqueous sodium hydroxide and oxygen gas. How much heat is released when 250.0 L of oxygen gas is produced from the reaction of sodium peroxide and water if the reaction is carried out in an open container at 1.000 atm pressure and 25°C?
(Given: DH°f[Na2O2(s)] = –510.9 kJ/mol; DH°f[NaOH(aq)] = –469.2 kJ/mol; DH°f[H2O(l)] = –285.8 kJ/mol)

  1. 141.7 kJ
    B. 1740 kJ
    C. 2900 kJ
    D. 3330 kJ
    E. 35,400 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: The Ideal Gas Law
Topic: Gases
Topic: Thermochemistry

 

 

 

At 25°C, the standard enthalpy of formation of anhydrous sodium carbonate is –1130.9 kJ/mol, whereas the standard enthalpy of formation of sodium carbonate monohydrate is –1430.1 kJ/mol. Determine DH° at 25°C for the reaction
Na2CO3(s) + H2O(l) ® Na2CO3·H2O(s).
(Given: DH°f[H2O(l)] = –285.8 kJ/mol)

  1. –585.0 kJ/mol
    B. –156.3 kJ/mol
    C. –299.2 kJ/mol
    D. –13.4 kJ/mol
    E. –285.8 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

  1. According to the first law of thermodynamics:
    A.Energy is neither lost nor gained in any energy transformations.
    B. Perpetual motion is possible.
    C. Energy is conserved in quality but not in quantity.
    D. Energy is being created as time passes. We have more energy in the universe now than when time began.

 

Bloom’s Level: 2. Understand
Difficulty: Easy
Gradable: automatic
Section: 06.03
Topic: Thermochemistry

 

 

 

  1. The heat of solution of KCl is 17.2 kJ/mol and the lattice energy of KCl(s) is 701.2 kJ/mol. Calculate the total heat of hydration of 1.00 mol of gas phase K+ ions and Cl ions.
    A.–718 kJ
    B. –684 kJ
    C. 684 kJ
    D. 718 kJ
    E. None of these.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.07
Topic: Thermochemistry

  1. The heat of solution of LiCl is –37.1 kJ/mol, and the lattice energy of LiCl(s) is 828 kJ/mol. Calculate the total heat of hydration of 1.00 mol of gas phase Li+ ions and Cl ions.
    A.–865 kJ
    B. –791 kJ
    C. 791 kJ
    D. 865 kJ
    E. None of these.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.07
Topic: Thermochemistry

 

 

  1. The total heat of hydration of 1.00 mol of gas phase Li+ ions and Cl ions is –865 kJ. The lattice energy of LiCl(s) is 828 kJ/mol. Calculate the heat of solution of LiCl.
    A.–1,693 kJ/mol
    B. –37 kJ/mol
    C. 37 kJ/mol
    D. 1,693 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.07
Topic: Thermochemistry

 

 

 

10.1 g CaO is dropped into a styrofoam coffee cup containing 157 g H2O at 18.0°C.
If the following reaction occurs, what temperature will the water reach, assuming that the cup is a perfect insulator and that the cup absorbs only a negligible amount of heat? (The specific heat of water = 4.18 J/g·°C)
CaO(s) + H2O(l) ® Ca(OH)2(s) DH°rxn = –64.8 kJ/mol

  1. 18.02°C
    B. 35.8°C
    C. 42.2°C
    D. 117°C
    E. 311°C

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: First Law of Thermodynamics (Conservation of Energy)
Topic: Thermochemistry

 

 

  1. The enthalpy change when a strong acid is neutralized by strong base is –56.1 kJ/mol. If 135 mL of 0.450 M HI at 23.15°C is mixed with 145 mL of 0.500 M NaOH, also at 23.15°C, what is the maximum temperature reached by the resulting solution? (Assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 J/g·°C, and that the density of the final solution is that of water.)
    A.20.24°C
    B. 26.06°C
    C. 29.19°C
    D. 32.35°C
    E. 36.57°C

 

Bloom’s Level: 3. Apply
Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Acid-Base Definitions
Subtopic: First Law of Thermodynamics (Conservation of Energy)
Topic: Acids and Bases
Topic: Thermochemistry

 

 

 

  1. The enthalpy change when a strong acid is neutralized by strong base is –56.1 kJ/mol. If 12.0 mL of 6.00 M HBr at 21.30°C is mixed with 300. mL of 0.250 M NaOH, also at 21.30°C, what is the maximum temperature reached by the resulting solution? (Assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 J/g·°C, and that the density of the final solution is that of water.)
    A.18.20°C
    B. 24.40°C
    C. 24.53°C
    D. 34.25°C
    E. 101.8°C

 

Bloom’s Level: 3. Apply
Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Acid-Base Definitions
Subtopic: First Law of Thermodynamics (Conservation of Energy)
Topic: Acids and Bases
Topic: Thermochemistry

 

 

  1. Calculate the amount of work done, in joules, when 2.5 mole of H2O vaporizes at 1.0 atm and 25°C. Assume the volume of liquid H2O is negligible compared to that of vapor. (1 L·atm = 101.3 J)
    A.61.1 J
    B. 518 J
    C. 5.66 kJ
    D. 6.19 kJ
    E. 6,190 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.03
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

  1. A gas is compressed in a cylinder from a volume of 20.0 L to 2.0 L by a constant pressure of 10.0 atm. Calculate the amount of work done on the system.
    A.–1.81 ´ 104 J
    B. –180 J
    C. 180 J
    D. 1.01 ´ 104 J
    E. 1.81 ´ 104 J

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.03
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. Calculate the amount of work done against an atmospheric pressure of 1.00 atm when 500.0 g of zinc dissolves in excess acid at 30.0°C.
    Zn(s) + 2H+(aq) ® Zn2+(aq) + H2(g)
    A.w = +22.4 kJ
    B. w = +24.9 kJ
    C. w = 0
    D. w = –2.52 kJ
    E. w = –19.3 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.03
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

A gas is allowed to expand, at constant temperature, from a volume of 1.0 L to 10.1 L against an external pressure of 0.50 atm. If the gas absorbs 250 J of heat from the surroundings, what are the values of q, w, and DE?

  1. A
    B. B
    C. C
    D. D
    E. E

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.03
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

  1. Which of the following processes always results in an increase in the energy of a system?
    A.The system loses heat and does work on the surroundings.
    B. The system gains heat and does work on the surroundings.
    C. The system loses heat and has work done on it by the surroundings.
    D. The system gains heat and has work done on it by the surroundings.
    E. None of these is always true.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.03
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

For which of these reactions will the difference between DH° and DE° be the greatest?

  1. 2H2O2(l) ® 2H2O(l) + O2(g)
    B. CaCO3(s) ® CaO(s) +CO2(g)
    C. NO(g) + O3(g) ® NO2(g) + O2(g)
    D. 2C2H6(g) + 7O2(g) ® 4CO2(g) + 6H2O(l)
    E. 4NH3(g) + 5O2(g) ® 4NO(g) + 6H2O(g)

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 06.04
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

For which of these reactions will the difference between DH° and DE° be the smallest?

  1. N2(g) + 3H2(g) ® 2NH3(g)
    B. 4PH3(g) ® P4(g) + 6H2(g)
    C. H2(g) + Cl2(g) ® 2HCl(g)
    D. CO2(g) + 2H2O(l) ® CH4(g) + 2O2(g)
    E. P4(s) + 10Cl2(g) ® 4PCl5(s)

 

Bloom’s Level: 5. Evaluate
Difficulty: Medium
Gradable: automatic
Section: 06.04
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

At 25°C, the following heats of reaction are known:

At the same temperature, use the above data to calculate the heat released (kJ) when 3.40 moles of ClF(g) reacts with excess F2:
ClF(g) + F2(g) ® ClF3(g)

  1. 109 kJ
    B. 233 kJ
    C. 370. kJ
    D. 465 kJ
    E. 1,580 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Hess’s Law
Topic: Thermochemistry

 

 

 

 

The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction
BrCl(g) ® Br(g) + Cl(g).
Use the following data to find the bond enthalpy of the Br–Cl bond.

  1. 14.6 kJ/mol
    B. 203.5 kJ/mol
    C. 219.0 kJ/mol
    D. 438.0 kJ/mol
    E. 407.0 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Hess’s Law
Topic: Thermochemistry

  1. The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH4NO3 is added to 40.0 mL of water in a calorimeter at 23.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 650. J/°C.)
    A.–7.7°C
    B. 14.3°C
    C. 20.8°C
    D. 21.4°C
    E. 25.6°C

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Calorimeter (Measuring Heats of Reactions)
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

 

 

  1. The heat of solution of ammonium chloride is 15.2 kJ/mol. If a 6.134 g sample of NH4Cl is added to 65.0 mL of water in a calorimeter at 24.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 365. J/°C.)
    A.18.6°C
    B. 19.7°C
    C. 21.9°C
    D. 27.1°C
    E. 30.4°C

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Calorimeter (Measuring Heats of Reactions)
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 12.5 g of aluminum is produced by this method. [DH°f(carbon monoxide) = –110.5 kJ/mol; DH°f(aluminum oxide) = –1669.8 kJ/mol]

  1. 310 kJ
    B. 361 kJ
    C. 697 kJ
    D. 725 kJ
    E. 1504 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Ozone (O3) in the atmosphere can be converted to oxygen gas by reaction with nitric oxide (NO). Nitrogen dioxide is also produced in the reaction. What is the enthalpy change when 8.50L of ozone at a pressure of 1.00 atm and 25°C reacts with 12.00 L of nitric oxide at the same initial pressure and temperature? [DH°f(NO) = 90.4 kJ/mol; DH°f(NO2) = 33.85 kJ/mol; DH°f(O3) = 142.2 kJ/mol]

  1. –1690 kJ
    B. –167 kJ
    C. –97.6 kJ
    D. –69.2 kJ
    E. –19.7 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Gas Stoichiometry
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Gases
Topic: Thermochemistry

 

True / False Questions

  1. Select True or False: Specific heat is defined as the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.
    TRUE

 

Bloom’s Level: 1. Remember
Difficulty: Easy
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Topic: Thermochemistry

 

 

 

 

Multiple Choice Questions

 

How many grams of ethylene (C2H4) would have to be burned to produce 450 kJ of heat?
C2H4(g) + 3O2(g) ® 2CO2(g) + H2O(l) DH°rxn = –1411 kJ/mol

  1. 5.95 g
    B. 695 g
    C. 7.95 g
    D. 8.95 g
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

Calculate the enthalpy of reaction for H2(g) + C2H4(g) ® C2H6(g).
[DH°f(C2H4(g)) = 52.3 kJ/mol; DH°f(C2H6(g)) = –84.7 kJ/mol]

  1. –117 kJ/mol
    B. –127 kJ/mol
    C. –137 kJ/mol
    D. –147 kJ/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

The enthalpy of combustion of acetylene C2H2 is described by
C2H2(g) + (5/2)O2(g) ® 2CO2(g) + H2O(l), DH°rxn= –1299 kJ/mol.
Calculate the enthalpy of formation of acetylene, given the following enthalpies of formation
DH°f[CO2(g)] = –393.5 kJ/mol
DH°f[H2O(l)] = –285.8 kJ/mol

  1. 216 kJ/mol
    B. 226 kJ/mol
    C. 236 kJ/mol
    D. 246 kJ/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Given the following DH° values,
H2(g) +  O2(g) ® H2O(l) DH°f = –285.8 kJ/mol
H2O2(l) ® H2(g) + O2(g) DH°rxn = 187.6 kJ/mol
calculate DH°rxn for the reaction H2O2(l) ® H2O(l) +  O2(g).

  1. –98.2 kJ/mol
    B. –88.2 kJ/mol
    C. –78.2 kJ/mol
    D. –68.2 kJ/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Hess’s Law
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

  1. The heat of solution of calcium chloride CaCl2 is –82.8 kJ/mol, and the combined heats of hydration of 1.00 mole of gaseous calcium ions and 2.00 mole of gaseous chloride ions is –2327 kJ. What is the lattice energy of calcium chloride?
    A.2,144 kJ/mol
    B. 2,244 kJ/mol
    C. 2,344 kJ/mol
    D. 2,444 kJ/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.07
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Hess’s Law
Topic: Thermochemistry

 

True / False Questions

  1. Select True or False: The heat of solution of NH4NO3 is 26.2 kJ/mol. Heat is evolved when a solution of NH4NO3 is diluted by addition of more water.
    FALSE

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.07
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

Multiple Choice Questions

  1. A 26.2 g piece of copper metal is heated from 21.5°C to 201.6°C. Calculate the amount of heat absorbed by the metal. The specific heat of Cu is 0.385 J/g·°C.
    A.1,620 J
    B. 1,720 J
    C. 1,820 J
    D. 1,920 J
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. A 0.1946 g piece of magnesium metal is burned in a constant-volume calorimeter that has a heat capacity of 1349 J/°C. The calorimeter contains 500. g of water and the temperature rise is 1.40°C. Calculate the heat of combustion of magnesium metal in kJ/g, given that the specific heat of water = 4.184 J/g·°C.
    A.21.8 kJ/g
    B. 22.8 kJ/g
    C. 23.8 kJ/g
    D. 24.8 kJ/g
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

  1. A 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000 kg of water contained therein rose from 20.22°C to 22.82°C. The heat capacity of the calorimeter is 2.21 kJ/°C. The heat capacity of water = 4.184 J/g·°C. How much heat was given off during combustion of the sample of pentane?
    A.18.6 kJ
    B. 17.6 kJ
    C. 16.6 kJ
    D. 15.6 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. A 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000 kg of water contained therein rose from 20.22°C to 22.82°C. The heat capacity of the calorimeter is 2.21 kJ/°C. The heat capacity of water = 4.184 J/g·°C. What is the heat of combustion, in kilojoules, per gram of pentane?
    A.48.6 kJ/g
    B. 47.6 kJ/g
    C. 46.6 kJ/g
    D. 45.6 kJ/g
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

  1. The heat of combustion of propane, C3H8, is 2220 kJ/mol. The specific heat of copper is 0.385 J/g´°C. How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings?
    A.3.36 g
    B. 3.26 g
    C. 3.16 g
    D. 3.06 g
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. The residential rate for natural gas is about $15 per thousand cubic foot. Burning one cubic foot of natural gas releases about 1080 kJ of heat. How much would it cost to heat the water in a 25,000 gallon swimming pool from 52°F to 78°F, assuming all of the heat from burning the natural gas went towards warming the water? (1 gal = 3.785 L; the specific heat of water = 4.184 J/g·°C)
    A.$69
    B. $79
    C. $89
    D. $99
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

The heat of neutralization of HCl by NaOH is DH°rxn = –56.2 kJ/mol. How much heat is released when 125 mL of 1.750 M HCl is mixed with 195 mL of 0.667 M NaOH?

  1. 7.11 kJ
    B. 7.21 kJ
    C. 7.31 kJ
    D. 7.41 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.04
Subtopic: Acid-Base Definitions
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Acids and Bases
Topic: Analyze
Topic: Thermochemistry

  1. The heat released when one mole of water is formed from the elements is 1,198 kJ. An experiment was conducted that permitted water to form in this manner, and the heat was contained in 2.0 liters of water. The water temperature before the reaction was 34.5°C, and after the reaction it had risen to 52.0°C. How many moles of water were formed? (The specific heat of water is 4.184 J/g·°C.)
    A.0.42 mole
    B. 0.32 mole
    C. 0.22 mole
    D. 0.12 mole
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

  1. When an automobile engine starts, the metal parts immediately begin to absorb heat released during the combustion of gasoline. How much heat will be absorbed by a 165 kg iron engine block as the temperature rises from 15.7°C to 95.7°C? (The specific heat of iron is 0.489 J/g·°C.)
    A.6,450 kJ
    B. 6,350 kJ
    C. 6,250 kJ
    D. 6,150 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

The value of DH°rxn for the following reaction is –6535 kJ/mol.
2C6H6(l) + 15O2(g) ® 12CO2(g) + 6H2O(g)
How many kilojoules of heat will be evolved during the combustion of 16.0 g of C6H6(l)?

  1. 689 kJ
    B. 679 kJ
    C. 669 kJ
    D. 659 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

What would be the standard enthalpy change for the reaction of 1.00 mole of H2(g) with 1.00 mole of Cl2(g) to produce 2.00 moles of HCl(g) at standard state conditions?
[DH°f (HCl(g))= –92.3 kJ/mol)]

  1. –155 kJ
    B. –165 kJ
    C. –175 kJ
    D. –185 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Calculate the heat released (kJ) in the reaction of 3.50 g of acetylene (C2H2) and excess hydrogen gas to form ethane gas:
C2H2(g) + 2H2(g) ® C2H6(g)
Given:
2C2H2(g) + 5O2(g) ® 4CO2(g) + 2H2O(g) DH = –2320 kJ/mol
2C2H6(g) + 7O2(g) ® 4CO2(g) + 6H2O(g) DH = –3040 kJ/mol
2H2(g) + O2(g) ® 2H2O(g) DH = –572 kJ/mol

  1. 27.5 kJ
    B. 28.5 kJ
    C. 29.5 kJ
    D. 30.5 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Hess’s Law
Topic: Thermochemistry

 

 

 

 

Calculate the heat released (kJ) in the reaction of 2.20 g of sulfur dioxide gas and excess oxygen gas to form sulfur trioxide gas:
2SO2(g) + O2(g) ® 2SO3(g)
Given:
S(s) + O2(g) ® SO2(g) DH = –299 kJ/mol
S(s) + 3/2O2(g) ® SO3(g) DH = –395 kJ/mol

  1. 3.10 kJ
    B. 3.20 kJ
    C. 3.30 kJ
    D. 3.40 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Hess’s Law
Topic: Thermochemistry

Find DH°rxn for the reaction
CH4(g) + 2O2(g) ® CO2(g) + 2H2O(l).
[DH°f (CH4(g)) = –74.8 kJ/mol; DH°f (CO2(g)) = –393.5 kJ/mol; DH°f (H2O(l)) = –285.5 kJ/mol]

  1. -879.7 kJ/mol
    B. -889.7 kJ/mol
    C. -899.7 kJ/mol
    D. -909.7 kJ/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

Find DH°rxn for the reaction
2Ag2S(s) + 2H2O(l) ® 4Ag(s) + 2H2S(g) + O2(g).
[DH°f (Ag2S(s)) = –32.6 kJ/mol; DH°f (H2S(g)) = –20.5 kJ/mol; DH°f (H2O(l)) = –285.5 kJ/mol]

  1. 595.2 kJ/mol
    B. 585.2 kJ/mol
    C. 575.2 kJ/mol
    D. 565.2 kJ/mol
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

Find DH°rxn for the reaction
2Na(s) + 2H2O(l) ® 2NaOH(aq) + 2H2(g).
[DH°f (NaOH(aq)) = –426.8 kJ/mol; DH°f (H2O(l)) = –285.5 kJ/mol]

  1. –284.6 kJ
    B. –282.6 kJ
    C. –280.6 kJ
    D. –278.6 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Subtopic: Standard Enthalpies of Formation and Reactions (
DH°f and DH°rxn)
Topic: Thermochemistry

 

 

 

 

  1. The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?
    A.240 J
    B. 250 J
    C. 260 J
    D. 270 J
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.05
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. At body temperature 2,404 joules of energy are required to evaporate 1.00 g of water. After vigorous exercise, a person feels chilly because the body is giving up heat to evaporate the perspiration. A typical person perspires 25 mL of water after 20. minutes of exercise. How much body heat is this person using to evaporate this water?
    A.6.0 ´ 104 J
    B. 6.3 ´ 104 J
    C. 6.5´ 104 J
    D. 6.7 ´ 104 J
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.04
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

  1. The combustion of one mole of benzene, C6H6, in oxygen liberates 3268 kJ of heat. The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?
    A.2290 kJ
    B. 2490 kJ
    C. 2690 kJ
    D. 2890 kJ
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.04
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

  1. A feverish student weighing 75 kilograms was immersed in 400. kg of water at 4.0°C to try to reduce the fever. The student’s body temperature dropped from 40.0°C to 37.0°C. Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?
    A.2.5°C
    B. 3.5°C
    C. 4.5°C
    D. 55°C
    E. None of the above

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

 

 

 

True / False Questions

 

  1. Select True or False: The specific heats of water and iron are 4.184 and 0.444 J/g°C, respectively. When equal masses of water and iron both absorb the same amount of heat, the temperature increase of the water will be 2.42 times greater than that of the iron.
    FALSE

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. Select True or False: Chemical reactions in a bomb calorimeter occur at constant pressure.
    TRUE

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.05
Subtopic: Calorimetry (Measuring Heats of Reaction)
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

Select True or False: If 2Mg(s) + O2(g) ® 2MgO(s), DH° = –1203.6 kJ/mol, then for
Mg(s) + (1/2)O2(g) ® MgO(s), the enthalpy change is DH = –601.8 kJ/mol.

TRUE

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.06
Subtopic: Enthalpy (Heats of Reaction)
Topic: Thermochemistry

 

 

 

 

  1. Select True or False: The heat capacity of 10.0 g of water is 83.7 J/°C.
    FALSE

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 06.05
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. Select True or False: The work done on the surroundings by the expansion of a gas is w = –PDV.
    TRUE

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.03
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

  1. Select True or False: The heat absorbed by a system at constant pressure is equal to DE – PDV.
    FALSE

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 06.04
Subtopic: System/Surroundings and Heat/work
Topic: Thermochemistry

 

Chapter 07

Quantum Theory and the Electronic Structure of Atoms

 

 

Multiple Choice Questions

In the following diagram of a wave

  1. (a) is amplitude and (b) is wavelength
    B. (a) is frequency and (b) is amplitude
    C. (a) is wavelength and (b) is frequency
    D. (a) is amplitude and (b) is frequency
    E. (a) is wavelength and (b) is amplitude

 

Bloom’s Level: 3. Apply
Difficulty: Easy
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Which of the following wavelengths of electromagnetic radiation has the highest energy?
    A.450. nm
    B. 225 nm
    C. 3.50 x 10-9 m
    D. 8.40 x 10-7 m
    E. 2.50 x 10-5 m

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. Which of the following frequencies of light has the highest energy?
    A.2.5 x 1010 s-1
    B. 7.0 x 1013 s-1
    C. 2.3 x 1014 s-1
    D. 5.0 x 1014 s-1
    E. 1.4 x 1015 s-1

 

Bloom’s Level: 3. Apply
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation

 

 

Topic: Quantum Theory and Atomic Structure

 

 

Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10-3 m.

  1. Gamma rays
    B. X rays
    C. Ultraviolet
    D. Infrared
    E. Microwave

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10-1 m.

  1. Gamma rays
    B. X rays
    C. Ultraviolet
    D. Infrared
    E. Microwave

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10-16 J/photon.

  1. Gamma rays
    B. X rays
    C. Ultraviolet
    D. Infrared
    E. Microwave

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10-18 J/photon.

  1. Gamma rays
    B. X rays
    C. Ultraviolet
    D. Infrared
    E. Microwave

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. What is the wavelength of radiation that has a frequency of 5.39 ´ 1014 s–1? (c = 2.9979 ´ 108 m/s)
    A.1.80 ´ 10–3 nm
    B. 556 nm
    C. 618 nm
    D. 6180 nm
    E. 1.61 ´ 1023 nm

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. What is the wavelength of radiation that has a frequency of 3.4 x 1011 s –1?
    A.8.8 x 10-4 nm
    B. 8.8 x 105 nm
    C. 8.8 x 10-13 nm
    D. 1.0 x 1011 nm
    E. 1.0 x 10-9 nm

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. Calculate the frequency of visible light having a wavelength of 486 nm.
    A.2.06 ´ 1014 /s
    B. 2.06 ´ 106 /s
    C. 6.17 ´ 1014 /s
    D. 1.20 ´ 10–15 /s
    E. 4.86 ´ 10–7 /s

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. Calculate the frequency of visible light having a wavelength of 686 nm.
    A.4.37 ´ 1014 /s
    B. 4.37 ´ 105 /s
    C. 6.17 ´ 1014 /s
    D. 2.29 ´ 10–15 /s
    E. 2.29 ´ 10–6 /s

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.01
Subtopic: Electromagnetic Radiation

 

 

Topic: Quantum Theory and Atomic Structure

 

 

  1. What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? (c = 2.9979 ´ 108 m/s; h = 6.626 ´ 10–34 J´s)
    A.2.70 ´ 10–43 J
    B. 5.43 ´ 10–33 J
    C. 1.63 ´ 10–24 J
    D. 4.07 ´ 10–10 J
    E. 2.46 ´ 109 J

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. What is the energy in joules of one photon of x-ray radiation with a wavelength of 0.120 nm?
    A.2.50 x 109 J
    B. 1.66 x 10-24 J
    C. 1.66 x 10-33 J
    D. 2.50 x 1018J
    E. 1.66 x 10-15J

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm?
    A.6.46 ´ 10–25 J
    B. 6.46 ´ 10–16 J
    C. 2.46 ´ 10–4 J
    D. 12.4 kJ
    E. 246 kJ

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 ´ 102 nm?
    A.4.72 ´ 10–43 J
    B. 1.71 ´ 105 J
    C. 12.4 kJ
    D. 256 kJ
    E. 2.12 ´ 1042 J

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 ´ 1014 /s?
    A.2.75 ´ 10–43 J/mol
    B. 1.66 ´ 10–19 J/mol
    C. 1.20 ´ 10–6 J/mol
    D. 99.7 kJ/mol
    E. 7.22 ´ 1017 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Subtopic: Planck’s Quantum Theory and Einstein’s Photoelectric Effect
Topic: Quantum Theory and Atomic Structure

  1. Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by
    En = –2.18 ´ 10–18 J(1/n2)
    A.2.07 ´ 10–29 J
    B. 2.25 ´ 10–18 J
    C. 2.04 ´ 10–18 J
    D. 3.27 ´ 10–17 J
    E. 2.19 ´ 105 J

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.03
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by
    En = –2.18 ´ 10–18 J(1/n2)
    A.9.18 ´ 10–20 nm
    B. 4.45 ´ 10–20 nm
    C. 2.16 ´ 10–6 nm
    D. 2.16 ´ 103 nm
    E. 1.38 ´ 1014 nm

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.03
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = –2.18 ´ 10–18 J(1/n2).
    A.1.82 ´ 10–19 /s
    B. 9.13 ´ 1013 /s
    C. 2.74 ´ 1014/s
    D. 3.65 ´ 1014 /s
    E. 1.64 ´ 1015 /s

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.03
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = –2.18 ´ 10 –18 J(1/n2).
    A.1.35 ´ 10–51 /s
    B. 1.03 ´ 108 /s
    C. 2.06 ´ 1014 /s
    D. 8.22 ´ 1014 /s
    E. 3.08 ´ 1015 /s

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.03
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = –2.18 ´ 10–18 J(1/n2).
    A.6.8 ´ 10–18 nm
    B. 0.612 nm
    C. 82.6 nm
    D. 97.2 nm
    E. 365 nm

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.03
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. The second line of the Balmer series occurs at a wavelength of 486.1 nm. What is the energy difference between the initial and final levels of the hydrogen atom in this emission process?
    A.2.44 ´ 1018 J
    B. 4.09 ´ 10–19 J
    C. 4.09 ´ 10–22 J
    D. 4.09 ´ 10–28 J
    E. 1.07 ´ 10–48 J

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.03
Subtopic: Atomic Spectra (Bohr Model of the Atom)
Subtopic: Electromagnetic Radiation
Topic: Quantum Theory and Atomic Structure

  1. A proton is roughly 1800 times more massive than an electron. If a proton and an electron are traveling at the same speed,
    A.the wavelength of the proton will be about 1800 times longer than the wavelength of the electron.
    B.

the wavelength of the proton will be about  times longer than the wavelength of the electron.

  1. the wavelength of the proton will be roughly equal to the wavelength of the electron.
    D.

the wavelength of the electron will be about  times longer than the wavelength of the proton.

  1. the wavelength of the electron will be about 1800 times longer than the wavelength of the proton.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. A proton is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy,
    A.the wavelength of the proton will be about 1800 times longer than the wavelength of the electron.
    B.

the wavelength of the proton will be about  times longer than the wavelength of the electron.

  1. the wavelength of the proton will be roughly equal to the wavelength of the electron.
    D.

the wavelength of the electron will be about  times longer than the wavelength of the proton.

  1. the wavelength of the electron will be about 1800 times longer than the wavelength of the proton.

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. If a hydrogen atom and a helium atom are traveling at the same speed,
    A.the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
    B. the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
    C. the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
    D. the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
    E. the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

  1. If a hydrogen atom and a helium atom have the same kinetic energy,
    A.the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
    B. the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
    C. the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
    D. the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
    E. the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling with a velocity of 7.0 ´ 103 kilometers per second. The mass of an electron is 9.1 ´ 10–28 g.
    A.1.0 ´ 10–13 m
    B. 1.0 ´ 10–10 m
    C. 1.0 ´ 10–7 m
    D. 1.0 m

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

  1. Calculate the wavelength associated with a 20Ne+ ion moving at a velocity of 2.0 ´ 105 m/s. The atomic mass of 20Ne is 19.992 amu.
    A.1.7 x 10-40 m
    B. 1.0 ´ 10–18 m
    C. 1.0 ´ 10–16 m
    D. 1.0 ´ 10–13 m
    E. 9.7 ´ 1012 m

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 ´ 10–24 g)
    A.1.6 pm
    B. 0.016 nm
    C. 0.16 nm
    D. 160 nm
    E. 1.6 ´ 10–4 m

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Quantum Theory and Atomic Structure

A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If DH for the reaction Cl2(g) ® 2Cl(g) is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution?

  1. 246.3 nm
    B. 349.3 nm
    C. 465.2 nm
    D. 492.6 nm
    E. 698.6 nm

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Subtopic: Planck’s Quantum Theory and Einstein’s Photoelectric Effect

 

 

Topic: Quantum Theory and Atomic Structure

 

 

  1. The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of wavelength 200. nm shines on a copper plate?
    A.1.97 ´ 104 m/s
    B. 4.67 ´ 104 m/s
    C. 6.22 ´ 105 m/s
    D. 1.34 ´ 106 m/s
    E. 1.48 ´ 106 m/s

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Subtopic: Planck’s Quantum Theory and Einstein’s Photoelectric Effect
Topic: Quantum Theory and Atomic Structure

  1. When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 ´ 105 m/s. Calculate the binding energy of electrons to the magnesium surface.
    A.32.7 kJ/mol
    B. 321 kJ/mol
    C. 353 kJ/mol
    D. 386 kJ/mol
    E. 419 kJ/mol

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Subtopic: Planck’s Quantum Theory and Einstein’s Photoelectric Effect
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Electrons can be used to probe the arrangement of atoms on a solid surface if the wavelength of the electrons is comparable with the spacing between the atoms. Which of the following electron velocities would be appropriate for use in this application if the atoms are separated by 0.320 nm?
    A.1.24 ´ 103 m/s
    B. 8.06 ´ 103 m/s
    C. 2.27 ´ 106 m/s
    D. 4.41 ´ 106 m/s
    E. 3.00 ´ 108 m/s

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.04
Subtopic: Electromagnetic Radiation
Subtopic: Planck’s Quantum Theory and Einstein’s Photoelectric Effect
Topic: Quantum Theory and Atomic Structure

  1. A single pulse of a laser yields an average of 5.00 ´ 1018 photons with l= 633 nm. If melting ice to water at 0°C requires 6.01 kJ/mol, what is the fewest number of laser pulses needed to melt 10.0 g of ice?
    A.38300
    B. 3830
    C. 3340
    D. 2120
    E. 212

 

Bloom’s Level: 4. Analyze
Difficulty: Difficult
Gradable: automatic
Section: 07.02
Subtopic: Electromagnetic Radiation
Subtopic: Planck’s Quantum Theory and Einstein’s Photoelectric Effect
Topic: Quantum Theory and Atomic Structure

 

 

 

 

Which one of the following sets of quantum numbers is not possible?

  1. A
    B. B
    C. C
    D. D
    E. E

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

 

 

 

 

Which one of the following sets of quantum numbers is not possible?

  1. A
    B. B
    C. C
    D. D
    E. E

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

  1. Which one of the following sets of quantum numbers represents an electron with the highest energy?
    A.n = 3, l = 2, ml = -2, ms = +1/2
    B. n = 4, l = 1, ml = 0, ms = -1/2
    C. n = 4, l = 0, ml = 0, ms = +1/2
    D. n = 5, l = 0, ml = 0, ms = +1/2
    E. n = 4, l = 2, ml = -1, ms = -1/2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.07
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Which one of the following sets of quantum numbers represents an electron with the highest energy?
    A.n = 2, l = 1, ml = 0, ms = +1/2
    B. n = 3, l = 0, ml = 0, ms = -1/2
    C. n = 2, l = 0, ml = 0, ms = +1/2
    D. n = 3, l = 2, ml = 1, ms = -1/2
    E. n = 3, l = 1, ml = 1, ms = +1/2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.07
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

  1. List the following sets of quantum numbers in order of increasing energy:
    I. n = 4, l = 1, ml = 1, ms = +1/2
    II. n = 3, l = 2, ml = -1, ms = +1/2
    III. n = 4, l = 0, ml = 0, ms = +1/2
    A.I < II < III
    B. II < III < I
    C. III < II < I
    D. I < III < II
    E. III < I < II

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.07
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. List the following sets of quantum numbers in order of increasing energy:
    I. n = 4, l = 0, ml = 0, ms = -1/2
    II. n = 4, l = 2, ml = -1, ms = -1/2
    III. n = 5, l = 0, ml = 0, ms = +1/2
    A.I < II < III
    B. II < III < I
    C. III < II < I
    D. I < III < II
    E. III < I < II

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.07
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

  1. Which of the following electronic transitions is consistent with an increase in energy?
    A.From a 4s subshell to a 3d subshell
    B. From a 5p subshell to a 4d subshell
    C. From a 4d subshell to a 5s subshell
    D. From a 4f subshell to a 6s subshell
    E. From a 5d subshell to a 6s subshell

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.07
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Which of the following electronic transitions is consistent with a decrease in energy?
    A.From a 5s subshell to a 4d subshell
    B. From a 4f subshell to a 5p subshell
    C. From a 6s subshell to a 5d subshell
    D. From a 5s subshell to a 5p subshell
    E. From a 4f subshell to a 6p subshell

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.07
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

  1. What is the maximum number of electrons in an atom that can have the following set of quantum numbers?
    n = 4 l = 3 ml = –2 ms = +1/2
    A.0
    B. 1
    C. 2
    D. 6
    E. 10

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.08
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. What is the maximum number of electrons in an atom that can have the following quantum numbers?
    n = 3 l = 2
    A.18
    B. 10
    C. 5
    D. 2
    E. 1

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Hund’s Rule
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

  1. What is the maximum number of electrons in an atom that can have the following set of quantum numbers?
    n = 3 l = 2 ml = –2
    A.18
    B. 10
    C. 5
    D. 2
    E. 1

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Hund’s Rule
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. What is the maximum number of electrons in an atom that can have the following quantum numbers?
    n = 3 l = 1
    A.18
    B. 6
    C. 3
    D. 2
    E. 1

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Hund’s Rule
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

  1. What is the maximum number of electrons in an atom that can have the following set of quantum numbers?
    n = 3 l = 1 ml = –1
    A.18
    B. 6
    C. 3
    D. 2
    E. 1

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

A possible set of quantum numbers for the last electron added to complete an atom of gallium (Ga) in its ground state is

  1. A
    B. B
    C. C
    D. D
    E. E

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.09
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

A possible set of quantum numbers for the last electron added to complete an atom of germanium (Ge) in its ground state is

  1. A
    B. B
    C. C
    D. D
    E. E

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.09
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

  1. A possible set of quantum numbers to describe an electron in a 4s subshell is
    A.n = 4, l = 0, ml = 1 , ms = +1/2
    B. n = 4, l = 0, ml = 0, ms = – 1/2
    C. n = 4, l = 1, ml = 1, ms = +1/2
    D. n = 3, l = 1, ml = 1, ms = – 1/2
    E. n = 3, l = 0, ml = 0, ms = +1/2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structur

 

 

 

 

  1. A possible set of quantum numbers to describe an electron in a 3d subshell is
    A.n = 3, l = 0, ml = 0 , ms = +1/2
    B. n = 3, l = 1, ml = 0, ms = – 1/2
    C. n = 3, l = 2, ml = 1, ms = +1/2
    D. n = 3, l = 3, ml = 1, ms = – 1/2
    E. n = 2, l = 0, ml = 0, ms = +1/2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

  1. A possible set of quantum numbers to describe an electron in a 5p subshell is
    A.n = 5, l = 2, ml = 2 , ms = +1/2
    B. n = 4, l = 0, ml = 0, ms = – 1/2
    C. n = 5, l = 0, ml = 0, ms = +1/2
    D. n = 3, l = 1, ml = 1, ms = – 1/2
    E. n = 5, l = 1, ml = 0, ms = +1/2

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

  1. Electrons in an orbital with l = 3 are in a/an
    A.d orbital.
    B. f orbital.
    C. g orbital.
    D. p orbital.
    E. s orbital.

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.06
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

  1. How many orbitals are allowed in a subshell if l = 3?
    A.1
    B. 3
    C. 5
    D. 7
    E. 9

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

 

 

4

 

  1. How many orbitals are allowed in a subshell if l = 2?
    A.1
    B. 3
    C. 5
    D. 7
    E. 9

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.06
Subtopic: Quantum Numbers
Topic: Quantum Theory and Atomic Structure

  1. “No two electrons in an atom can have the same four quantum numbers” is a statement of
    A.the Pauli exclusion principle.
    B. Bohr’s equation.
    C. Hund’s rule.
    D. de Broglie’s relation.
    E. Dalton’s atomic theory.

 

Bloom’s Level: 4. Analyze
Difficulty: Easy
Gradable: automatic
Section: 07.08
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Mechanics (Wave-Particle Duality and the Heisenberg Uncertainty Principle)
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

The orbital diagram for a ground-state nitrogen atom is

  1. A
    B. B
    C. C
    D. D

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

The orbital diagram for a ground-state oxygen atom is

  1. A
    B. B
    C. C
    D. D
    E. E

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure

 

 

 

 

The orbital diagram for a ground state carbon atom is

  1. A
    B. B
    C. C
    D. D

 

Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 07.08
Subtopic: Assigning Electrons to Atomic Orbitals (Aufbau Principle)
Subtopic: Hund’s Rule
Subtopic: Pauli Exclusion Principle
Subtopic: Quantum Numbers
Topic: Electron Configuration
Topic: Quantum Theory and Atomic Structure