Question 1

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

Accepted Answer

A)   at low temperature, the reaction is spontaneous and ΔG 
B)   at low temperature, the reaction is nonspontaneous and ΔG > 0 and at high temperature, the reaction is spontaneous and ΔG 
C)   at low 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.F) All of the above
G) A) and C)

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)   FourthF) None of the above
G) C) and E)

Question 3

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 kJF) B) and D)
G) None of the above

Question 4

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) F) C) and E)
G) B) and E)

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/KF) A) and D)
G) B) and E)

Question 6

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 × 104F) B) and D)
G) All of the above

Question 7

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.F) None of the above
G) C) and D)

Question 8

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 kJF) A) and D)
G) C) and E)

Question 9

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.F) B) and C)
G) C) and D)

Question 10

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/KF) B) and D)
G) B) and C)

Exam 18: Free Energy and Thermodynamics

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

Correct Answer
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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.

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

Correct Answer
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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

Correct Answer
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Identify the compound with the highest ΔG°_f.

Correct Answer
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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

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

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

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

Correct Answer
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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

Correct Answer
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Exam 18: Free Energy and Thermodynamics

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

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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.

Correct AnswerverifiedShow Answer

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

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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

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Identify the compound with the highest ΔG°f.

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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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

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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

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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

Correct Answer
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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.

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

Correct Answer
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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

Correct Answer
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Identify the compound with the highest ΔG°_f.

Correct Answer
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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

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

Correct Answer
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Correct Answer
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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

Correct Answer
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