Question 1

Determine the equilibrium constant for the following reaction at 298 K. N2(g) + O2(g) → 2 NO(g) ΔG° = 173.3 kJ

Accepted Answer

A)   5.31 × 10-15
B)   4.19 × 10-31
C)   6.03 × 10-6
D)   1.32 × 10-22
E)   2.42× 10-11F) B) and D)
G) B) and E)

Question 2

Identify the compound with the lowest standard free energy of formation.

Accepted Answer

A)   NaCl(s) 
B)   O2(g) 
C)   NO(g) 
D)   O3(g) 
E)   It is hard to determine.F) C) and D)
G) A) and B)

Question 3

Identify the change in state that does not have an increase in entropy.

Accepted Answer

A)   gasoline freezing
B)   water boiling
C)   ice melting
D)   dry ice subliming
E)   water evaporatingF) B) and C)
G) A) and E)

Question 4

How is a nonspontaneous process made spontaneous?

Accepted Answer

The nonspontaneous p...

Question 5

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) A) and E)
G) None of the above

Question 6

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

Accepted Answer

A)   Zero
B)   First
C)   Second
D)   Third
E)   FourthF) A) and C)
G) C) and E)

Question 7

Under which of the following conditions would one mole of Ne have the highest entropy,S?

Accepted Answer

A)   27°C and 25 L
B)   137°C and 25 L
C)   27°C and 35 L
D)   137°C and 35 LE) A) and D)
F) A) and B)

Question 8

Identify the process that is spontaneous

Accepted Answer

A)   rusting of iron
B)   electrolysis
C)   photosynthesis
D)   water flowing uphill
E)   burning gasolineF) A) and E)
G) A) and B)

Question 9

Place the following in order of increasing molar entropy at 298 K. NO CO SO

Accepted Answer

A)   NO 
B)   SO 
C)   SO 
D)   CO 
E)   CO < NO < SOF) C) and D)
G) B) and D)

Question 10

Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔG°rxn = ?
ΔH°f (kJ/mol) -20.6 -296.8 -241.8
S°(J/mol∙K) 205.8 205.2 248.2 188.8

Accepted Answer

A)   -990.3 kJ
B)   +108.2 kJ
C)   -466.1 kJ
D)   +676.2 kJ
E)   -147.1 kJF) C) and E)
G) A) and D)

Question 11

Which one of the following has the highest standard molar entropy,S°,at 25°C?

Accepted Answer

A)   I2(g) 
B)   F2(g) 
C)   Br2(l) 
D)   H2(g) 
E)   Cl2(g) F) A) and B)
G) B) and C)

Question 12

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ
P(Hg) = 0.025 atm,P(O2) = 0.037 atm

Accepted Answer

A)   +207 kJ
B)   -154.4 kJ
C)   -26.5 kJ
D)   -164 kJ
E)   +60.7 kJF) All of the above
G) A) and B)

Question 13

Above what temperature does the following reaction become nonspontaneous?
FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH = -11.0 kJ; ΔS = -17.4 J/K

Accepted Answer

A)   632 K
B)   298 K
C)   191 K
D)   This reaction is nonspontaneous at all temperatures.
E)   This reaction is spontaneous at all temperatures.F) A) and B)
G) C) and E)

Question 14

Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) K = ?
ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1

Accepted Answer

A)   8.71 × 108
B)   0.980
C)   1.15 × 10-9
D)   1.02
E)   5.11 × 10-4F) A) and B)
G) A) and C)

Question 15

Above what temperature does the following reaction become nonspontaneous?
N2(s) + 3 H2(g) → 2 NH3(g) ΔH = -92.22 kJ; ΔS = -198.75 J/K

Accepted Answer

A)   186 K
B)   326 K
C)   464 K
D)   This reaction is nonspontaneous at all temperatures.
E)   This reaction is spontaneous at all temperatures.F) A) and E)
G) A) and B)

Question 16

Why is heating your home with gas more efficient than heating it with electricity?

Accepted Answer

Heating with gas only requires a one ste...

Question 17

Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ
Calculate ΔG°rxn for the following reaction.
3 C3H8(g) + 15 O2(g) → 9 CO2(g) + 12 H2O(g)

Accepted Answer

A)   -2074 kJ
B)   + 6222 kJ
C)   - 6222 kJ
D)   +2074 kJ
E)   - 691 kJF) B) and D)
G) A) and B)

Question 18

Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ
Calculate ΔG°rxn for the following reaction.
12 CO2(g) + 16 H2O(g) → 4 C3H8(g) + 20 O2 g)

Accepted Answer

A)   -2074 kJ
B)   + 8296 kJ
C)   - 8296 kJ
D)   +2074 kJ
E)   - 518 kJF) D) and E)
G) A) and E)

Question 19

Match between columns Premises: Q = K Q < 1 Q < K Q > 1 Q > K Q = 1

Accepted Answer

The Answer of K = 0 and ΔG < ΔG° is...

Question 20

Estimate ΔG°rxn for the following reaction at 875 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH°= -304.2 kJ; ΔS°= -414.2 J/K

Accepted Answer

A)   -2.63 kJ
B)   - 58.0 kJ
C)   + 58.0 kJ
D)   + 666 kJ
E)   - 666 kJF) C) and D)
G) A) and C)

Exam 19: Free Energy and Thermodynamics

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

Correct Answer
verified

Given the following equation, C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔG°_rxn = -2074 kJ Calculate ΔG°_rxn for the following reaction. 3 C₃H₈(g) + 15 O₂(g) → 9 CO₂(g) + 12 H₂O(g)

Correct Answer
verified

Identify the compound with the lowest standard free energy of formation.

Correct Answer
verified

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

Correct Answer
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Given the following equation, C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔG°_rxn = -2074 kJ Calculate ΔG°_rxn for the following reaction. 12 CO₂(g) + 16 H₂O(g) → 4 C₃H₈(g) + 20 O₂ g)

Correct Answer
verified

Which one of the following has the highest standard molar entropy,S°,at 25°C?

Correct Answer
verified

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O₂) = 0.037 atm

Correct Answer
verified

Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO₂(g) + Fe(s) ΔH = -11.0 kJ; ΔS = -17.4 J/K

Correct Answer
verified

Identify the process that is spontaneous

Correct Answer
verified

Place the following in order of increasing molar entropy at 298 K. NO CO SO

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 298 K. N₂(g) + O₂(g) → 2 NO(g) ΔG° = 173.3 kJ

Correct Answer
verified

How is a nonspontaneous process made spontaneous?

Correct Answer
verified
The nonspontaneous p...
View Answer

Match the following.

Why is heating your home with gas more efficient than heating it with electricity?

Correct Answer
verified
Heating with gas only requires a one ste...
View Answer

Estimate ΔG°_rxn for the following reaction at 875 K. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔH°= -304.2 kJ; ΔS°= -414.2 J/K

Correct Answer
verified

Under which of the following conditions would one mole of Ne have the highest entropy,S?

Correct Answer
verified

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔH°_f (kJ/mol) -20.6 -296.8 -241.8 S°(J/mol^∙K) 205.8 205.2 248.2 188.8

Correct Answer
verified

Above what temperature does the following reaction become nonspontaneous? N₂(s) + 3 H₂(g) → 2 NH₃(g) ΔH = -92.22 kJ; ΔS = -198.75 J/K

Correct Answer
verified

Identify the change in state that does not have an increase in entropy.

Correct Answer
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Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) K= ? ΔG°_f (kJ/mol) -110.9 87.6 51.3 -237.1

Correct Answer
verified

Exam 19: Free Energy and Thermodynamics

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

Correct AnswerverifiedShow Answer

Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ Calculate ΔG°rxn for the following reaction. 3 C3H8(g) + 15 O2(g) → 9 CO2(g) + 12 H2O(g)

Correct AnswerverifiedShow Answer

Identify the compound with the lowest standard free energy of formation.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ Calculate ΔG°rxn for the following reaction. 12 CO2(g) + 16 H2O(g) → 4 C3H8(g) + 20 O2 g)

Correct AnswerverifiedShow Answer

Which one of the following has the highest standard molar entropy,S°,at 25°C?

Correct AnswerverifiedShow Answer

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O2) = 0.037 atm

Correct AnswerverifiedShow Answer

Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH = -11.0 kJ; ΔS = -17.4 J/K

Correct AnswerverifiedShow Answer

Identify the process that is spontaneous

Correct AnswerverifiedShow Answer

Place the following in order of increasing molar entropy at 298 K. NO CO SO

Correct AnswerverifiedShow Answer

Determine the equilibrium constant for the following reaction at 298 K. N2(g) + O2(g) → 2 NO(g) ΔG° = 173.3 kJ

Correct AnswerverifiedShow Answer

How is a nonspontaneous process made spontaneous?

Correct AnswerverifiedThe nonspontaneous p...View AnswerShow Answer

Match the following.

Why is heating your home with gas more efficient than heating it with electricity?

Correct AnswerverifiedHeating with gas only requires a one ste...View AnswerShow Answer

Estimate ΔG°rxn for the following reaction at 875 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH°= -304.2 kJ; ΔS°= -414.2 J/K

Correct AnswerverifiedShow Answer

Under which of the following conditions would one mole of Ne have the highest entropy,S?

Correct AnswerverifiedShow Answer

Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔG°rxn = ? ΔH°f (kJ/mol) -20.6 -296.8 -241.8 S°(J/mol∙K) 205.8 205.2 248.2 188.8

Correct AnswerverifiedShow Answer

Above what temperature does the following reaction become nonspontaneous? N2(s) + 3 H2(g) → 2 NH3(g) ΔH = -92.22 kJ; ΔS = -198.75 J/K

Correct AnswerverifiedShow Answer

Identify the change in state that does not have an increase in entropy.

Correct AnswerverifiedShow Answer

Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) K = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1

Correct AnswerverifiedShow Answer

Correct Answer
verified

Given the following equation, C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔG°_rxn = -2074 kJ Calculate ΔG°_rxn for the following reaction. 3 C₃H₈(g) + 15 O₂(g) → 9 CO₂(g) + 12 H₂O(g)

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Given the following equation, C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔG°_rxn = -2074 kJ Calculate ΔG°_rxn for the following reaction. 12 CO₂(g) + 16 H₂O(g) → 4 C₃H₈(g) + 20 O₂ g)

Correct Answer
verified

Correct Answer
verified

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O₂) = 0.037 atm

Correct Answer
verified

Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO₂(g) + Fe(s) ΔH = -11.0 kJ; ΔS = -17.4 J/K

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 298 K. N₂(g) + O₂(g) → 2 NO(g) ΔG° = 173.3 kJ

Correct Answer
verified

Correct Answer
verified
The nonspontaneous p...
View Answer

Correct Answer
verified
Heating with gas only requires a one ste...
View Answer

Estimate ΔG°_rxn for the following reaction at 875 K. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔH°= -304.2 kJ; ΔS°= -414.2 J/K

Correct Answer
verified

Correct Answer
verified

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔH°_f (kJ/mol) -20.6 -296.8 -241.8 S°(J/mol^∙K) 205.8 205.2 248.2 188.8

Correct Answer
verified

Above what temperature does the following reaction become nonspontaneous? N₂(s) + 3 H₂(g) → 2 NH₃(g) ΔH = -92.22 kJ; ΔS = -198.75 J/K

Correct Answer
verified

Correct Answer
verified

Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) K= ? ΔG°_f (kJ/mol) -110.9 87.6 51.3 -237.1

Correct Answer
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