Question 1

Identify the compound with the highest ΔG°f.

Accepted Answer

A)  N2(g) 
B)  H2(g) 
C)  O2(g) 
D)  Cl2(g) 
E)  All compounds have a value of zero. 
A)  N2(g) 
B)  H2(g) 
C)  O2(g) 
D)  Cl2(g) 
E)  All compounds have a value of zero.

Question 2

The ________ Law of Thermodynamics states the energy is conserved in chemical processes.

Accepted Answer

A)  Zero 
B)  First 
C)  Second 
D)  Third 
E)  Fourth 
A)  Zero 
B)  First 
C)  Second 
D)  Third 
E)  Fourth

Question 3

The value of ΔG° at 100.0°C for the formation of calcium chloride from its constituent elements: Ca(s)+ Cl2(g)→ CaCl2(s)
Is ________ kJ/mol.At 25.0°C for this reaction,ΔH° is -795.8 kJ/mol,ΔG° is -748.1 kJ/mol,and ΔS° is -159.8 J/K.

Accepted Answer

A)  -855.4 
B)  -736.1 
C)  5.88 × 104 
D)  -779.8 
E)  1.52 × 104 
A)  -855.4 
B)  -736.1 
C)  5.88 × 104 
D)  -779.8 
E)  1.52 × 104

Question 4

Use Hess's law to calculate ΔG°rxn using the following information. NO(g)+ O(g)→ NO2(g)ΔG°rxn = ?
2 O3(g)→ 3 O2(g)ΔG°rxn = +489.6 kJ
O2(g)→ 2 O(g)ΔG°rxn = +463.4 kJ
NO(g)+ O3(g)→ NO2(g)+ O2(g)ΔG°rxn = -199.5 kJ

Accepted Answer

A)  +753.5 kJ 
B)  +277.0 kJ 
C)  -676.0 kJ 
D)  -1152.5 kJ 
E)  -225.7 kJ 
A)  +753.5 kJ 
B)  +277.0 kJ 
C)  -676.0 kJ 
D)  -1152.5 kJ 
E)  -225.7 kJ

Question 5

Calculate DS°rxn for the following reaction.The S° for each species is shown below the reaction. P4(g)+ 10 Cl2(g)→ 4 PCl5(g)
S°(J/mol∙K)280.0 223.1 364.6

Accepted Answer

A)  +138.5 J/K 
B)  -1052.6 J/K 
C)  -171.3 J/K 
D)  -583.6 J/K 
E)  -307.7 J/K 
A)  +138.5 J/K 
B)  -1052.6 J/K 
C)  -171.3 J/K 
D)  -583.6 J/K 
E)  -307.7 J/K

Question 6

Calculate ΔS°rxn for the following reaction.The S° for each species is shown below the reaction. C2H2(g)+ H2(g)→ C2H4(g)
S°(J/mol∙K)200.9 130.7 219.3

Accepted Answer

A)  +112.3 J/K 
B)  +550.9 J/K 
C)  -112.3 J/K 
D)  +337.1 J/K 
E)  -550.9 J/K 
A)  +112.3 J/K 
B)  +550.9 J/K 
C)  -112.3 J/K 
D)  +337.1 J/K 
E)  -550.9 J/K

Question 7

Place the following in order of increasing standard molar entropy. H2O(l)H2O(g)H2O(s)

Accepted Answer

A)  H2O(g) 2O(l) 2O(s) 
B)  H2O(s) 2O(l) 2O(g) 
C)  H2O(g) 2O(s) 2O(l) 
D)  H2O(l) 2O(s) 2O(g) 
E)  H2O(s) 2O(g) 2O(l) 
A)  H2O(g) 2O(l) 2O(s) 
B)  H2O(s) 2O(l) 2O(g) 
C)  H2O(g) 2O(s) 2O(l) 
D)  H2O(l) 2O(s) 2O(g) 
E)  H2O(s) 2O(g) 2O(l)

Question 8

Which of the following reactions will have the largest equilibrium constant (K)at 298 K?

Accepted Answer

A)  CaCO3(s) → CaO(s) + CO2(g) ΔG° =+131.1 kJ 
B)  2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ 
C)  3 O2(g) → 2 O3(g) ΔG° = +326 kJ 
D)  Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ 
E)  It is not possible to determine without more information. 
A)  CaCO3(s) → CaO(s) + CO2(g) ΔG° =+131.1 kJ 
B)  2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ 
C)  3 O2(g) → 2 O3(g) ΔG° = +326 kJ 
D)  Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ 
E)  It is not possible to determine without more information.

Question 9

Estimate ΔG°rxn for the following reaction at 417 K. HCN(g)+ 2 H2(g)→ CH3NH2(g)ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

Accepted Answer

A)  +61.9 kJ 
B)  -66.3 kJ 
C)  +66.3 kJ 
D)  -250 kJ 
E)  +250 kJ 
A)  +61.9 kJ 
B)  -66.3 kJ 
C)  +66.3 kJ 
D)  -250 kJ 
E)  +250 kJ

Question 10

For the following example,identify the following. F2(l)→ F2(g)

Accepted Answer

A)  at low temperature, the reaction is spontaneous and ΔG  0 and at high temperature, the reaction is spontaneous and ΔG  0 
D)  at low temperature, the reaction is nonspontaneous and ΔG > 0 and at high temperature, the reaction is nonspontaneous and ΔG > 0 
E)  It is not possible to determine without more information. 
A)  at low temperature, the reaction is spontaneous and ΔG  0 and at high temperature, the reaction is spontaneous and ΔG  0 
D)  at low temperature, the reaction is nonspontaneous and ΔG > 0 and at high temperature, the reaction is nonspontaneous and ΔG > 0 
E)  It is not possible to determine without more information.

Identify the compound with the highest ΔG°_f.

The ________ Law of Thermodynamics states the energy is conserved in chemical processes.

The value of ΔG° at 100.0°C for the formation of calcium chloride from its constituent elements: Ca(s)+ Cl₂(g)→ CaCl₂(s) Is ________ kJ/mol.At 25.0°C for this reaction,ΔH° is -795.8 kJ/mol,ΔG° is -748.1 kJ/mol,and ΔS° is -159.8 J/K.

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g)+ O(g)→ NO₂(g)ΔG°_rxn= ? 2 O₃(g)→ 3 O₂(g)ΔG°_rxn= +489.6 kJ O₂(g)→ 2 O(g)ΔG°_rxn= +463.4 kJ NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)ΔG°_rxn= -199.5 kJ

Calculate DS°_rxn for the following reaction.The S° for each species is shown below the reaction. P₄(g)+ 10 Cl₂(g)→ 4 PCl₅(g) S°(J/mol∙K)280.0 223.1 364.6

Calculate ΔS°_rxn for the following reaction.The S° for each species is shown below the reaction. C₂H₂(g)+ H₂(g)→ C₂H₄(g) S°(J/mol∙K)200.9 130.7 219.3

Place the following in order of increasing standard molar entropy. H₂O(l)H₂O(g)H₂O(s)

Which of the following reactions will have the largest equilibrium constant (K)at 298 K?

Estimate ΔG°_rxn for the following reaction at 417 K. HCN(g)+ 2 H₂(g)→ CH₃NH₂(g)ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

For the following example,identify the following. F₂(l)→ F₂(g)

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Exam 18: Free Energy and Thermodynamics

Identify the compound with the highest ΔG°f.

The ________ Law of Thermodynamics states the energy is conserved in chemical processes.

The value of ΔG° at 100.0°C for the formation of calcium chloride from its constituent elements: Ca(s)+ Cl2(g)→ CaCl2(s) Is ________ kJ/mol.At 25.0°C for this reaction,ΔH° is -795.8 kJ/mol,ΔG° is -748.1 kJ/mol,and ΔS° is -159.8 J/K.

Use Hess's law to calculate ΔG°rxn using the following information. NO(g)+ O(g)→ NO2(g)ΔG°rxn = ? 2 O3(g)→ 3 O2(g)ΔG°rxn = +489.6 kJ O2(g)→ 2 O(g)ΔG°rxn = +463.4 kJ NO(g)+ O3(g)→ NO2(g)+ O2(g)ΔG°rxn = -199.5 kJ

Calculate DS°rxn for the following reaction.The S° for each species is shown below the reaction. P4(g)+ 10 Cl2(g)→ 4 PCl5(g) S°(J/mol∙K)280.0 223.1 364.6

Calculate ΔS°rxn for the following reaction.The S° for each species is shown below the reaction. C2H2(g)+ H2(g)→ C2H4(g) S°(J/mol∙K)200.9 130.7 219.3

Place the following in order of increasing standard molar entropy. H2O(l)H2O(g)H2O(s)

Which of the following reactions will have the largest equilibrium constant (K)at 298 K?

Estimate ΔG°rxn for the following reaction at 417 K. HCN(g)+ 2 H2(g)→ CH3NH2(g)ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

For the following example,identify the following. F2(l)→ F2(g)

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

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Chemical Kinetics

Chemical Equilibrium

Acids and Bases

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Identify the compound with the highest ΔG°_f.

The value of ΔG° at 100.0°C for the formation of calcium chloride from its constituent elements: Ca(s)+ Cl₂(g)→ CaCl₂(s) Is ________ kJ/mol.At 25.0°C for this reaction,ΔH° is -795.8 kJ/mol,ΔG° is -748.1 kJ/mol,and ΔS° is -159.8 J/K.

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g)+ O(g)→ NO₂(g)ΔG°_rxn= ? 2 O₃(g)→ 3 O₂(g)ΔG°_rxn= +489.6 kJ O₂(g)→ 2 O(g)ΔG°_rxn= +463.4 kJ NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)ΔG°_rxn= -199.5 kJ

Calculate DS°_rxn for the following reaction.The S° for each species is shown below the reaction. P₄(g)+ 10 Cl₂(g)→ 4 PCl₅(g) S°(J/mol∙K)280.0 223.1 364.6

Calculate ΔS°_rxn for the following reaction.The S° for each species is shown below the reaction. C₂H₂(g)+ H₂(g)→ C₂H₄(g) S°(J/mol∙K)200.9 130.7 219.3

Place the following in order of increasing standard molar entropy. H₂O(l)H₂O(g)H₂O(s)

Estimate ΔG°_rxn for the following reaction at 417 K. HCN(g)+ 2 H₂(g)→ CH₃NH₂(g)ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

For the following example,identify the following. F₂(l)→ F₂(g)