Question 1

How is a nonspontaneous process made spontaneous?

Accepted Answer

The nonspontaneous process is coupled wi...

Question 2

Which of the following is NOT true for ΔGrxn?

Accepted Answer

A)   If ΔG°rxn > 0, the reaction is spontaneous in the forward direction.
B)   If Q = 1, then DGrxn = ΔG°rxn.
C)   If ΔG°rxn 
D)   If ΔG°rxn > 0, the reaction is spontaneous in the reverse direction.
E)   Under equilibrium conditions, ΔGrxn = 0.

Question 3

Place the following in order of decreasing molar entropy at 298 K. H2 Cl2 F2

Accepted Answer

A)   H2 > Cl2 > F2
B)   Cl2 > H2 > F2
C)   F2 > Cl2 > H2
D)   H2 > F2 > Cl2
E)   Cl2 > F2 > H2

Question 4

A spontaneous reaction occurs

Accepted Answer

A)   with expansion of the volume.
B)   with the application of cold.
C)   with the application of heat.
D)   without ongoing outside intervention.
E)   with a catalyst.

Question 5

What is true if ln K is 1?

Accepted Answer

A)   ΔG°rxn is positive and the reaction is spontaneous in the forward direction.
B)   ΔG°rxn is negative and the reaction is spontaneous in the forward direction.
C)   ΔG°rxn is negative and the reaction is spontaneous in the reverse direction.
D)   ΔG°rxn is positive and the reaction is spontaneous in the reverse direction.
E)   ΔG°rxn is zero and the reaction is at equilibrium.

Question 6

Define entropy.

Accepted Answer

Entropy is a thermodynamic fun...

Question 7

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ
P(O2) = 0.41 atm,P(O3) = 5.2 atm

Accepted Answer

A)   +341 kJ
B)   +17.8 kJ
C)   +332 kJ
D)   -47.4 kJ
E)   -109 kJ

Question 8

An endothermic reaction is a process that

Accepted Answer

A)   has a negative ΔHsys and a positive ΔSsurr.
B)   has a negative ΔHsys and a negative ΔSsurr.
C)   has a positive ΔHsys and a positive ΔSsurr.
D)   has a positive ΔHsys and a negative ΔSsurr.

Question 9

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ
Calculate ΔG°rxn for the following reaction.
6 N2O(g) + 6 NO2(g) → 18 NO(g)

Accepted Answer

A)   -23.0 kJ
B)   138 kJ
C)   -138 kJ
D)   -3.83 kJ
E)   23.0 kJ

Question 10

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

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.

Question 11

Why is the quantity of energy required to recharge a battery greater than the quantity of work done?

Accepted Answer

Some of th...

Question 12

Calculate ΔS°rxn for the following reaction.The S° for each species is shown below the reaction. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) 
S°(J/mol∙K) 192.8 205.2 210.8 188.8

Accepted Answer

A)   -287.4 J/K
B)   -401.2 J/K
C)   +160.0 J/K
D)   +336.6 J/K
E)   +178.8 J/K

Question 13

Estimate ΔG°rxn for the following reaction at 449.0 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K

Accepted Answer

A)   +5.8 kJ
B)   -12.9 kJ
C)   -101 kJ
D)   -5.8 kJ
E)   -4.2 kJ

Question 14

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K

Accepted Answer

A)   6.762 × 103 K
B)   158.7 K
C)   298 K
D)   This reaction is nonspontaneous at all temperatures.
E)   This reaction is spontaneous at all temperatures.

Question 15

Define allotrope.

Accepted Answer

Allotropes are diffe...

Question 16

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 kJ

Question 17

For a given compound,list the decreasing order of entropy for a liquid,solid,and gas.

Accepted Answer

A)   solid > gas > liquid
B)   liquid > solid > gas
C)   gas > liquid > solid
D)   gas > solid > liquid
E)   solid > liquid > gas

Question 18

Calculate ΔS°rxn for the following reaction.The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) 
S° (J/mol∙K) 121.2 130.7 192.8

Accepted Answer

A)   +133.7 J/K
B)   -59.1 J/K
C)   +118.2 J/K
D)   +202.3 J/K
E)   -444.7 J/K

Question 19

Consider a reaction that has a negative ΔH and a negative ΔS.Which of the following statements is TRUE?

Accepted Answer

A)   This reaction will be spontaneous only at high temperatures.
B)   This reaction will be spontaneous at all temperatures.
C)   This reaction will be nonspontaneous at all temperatures.
D)   This reaction will be nonspontaneous only at high temperatures.
E)   It is not possible to determine without more information.

Question 20

For the following example,identify the following. 2 F2O(g) → 2 F2(g) + O2(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.

Exam 18: Free Energy and Thermodynamics

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

Define allotrope.

Correct AnswerverifiedAllotropes are diffe...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

Which of the following is NOT true for ΔGrxn?

Correct AnswerverifiedShow Answer

For the following example,identify the following. 2 F2O(g) → 2 F2(g) + O2(g)

Correct AnswerverifiedShow Answer

Consider a reaction that has a negative ΔH and a negative ΔS.Which of the following statements is TRUE?

Correct AnswerverifiedShow Answer

A spontaneous reaction occurs

Correct AnswerverifiedShow Answer

For a given compound,list the decreasing order of entropy for a liquid,solid,and gas.

Correct AnswerverifiedShow Answer

Why is the quantity of energy required to recharge a battery greater than the quantity of work done?

Correct AnswerverifiedSome of th...View AnswerShow Answer

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.41 atm,P(O3) = 5.2 atm

Correct AnswerverifiedShow Answer

Place the following in order of decreasing molar entropy at 298 K. H2 Cl2 F2

Correct AnswerverifiedShow Answer

Define entropy.

Correct AnswerverifiedEntropy is a thermodynamic fun...View AnswerShow Answer

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K

Correct AnswerverifiedShow Answer

Calculate ΔS°rxn for the following reaction.The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) S° (J/mol∙K) 121.2 130.7 192.8

Correct AnswerverifiedShow Answer

Estimate ΔG°rxn for the following reaction at 449.0 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K

Correct AnswerverifiedShow Answer

Calculate ΔS°rxn for the following reaction.The S° for each species is shown below the reaction. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) S°(J/mol∙K) 192.8 205.2 210.8 188.8

Correct AnswerverifiedShow Answer

What is true if ln K is 1?

Correct AnswerverifiedShow Answer

An endothermic reaction is a process that

Correct AnswerverifiedShow Answer

How is a nonspontaneous process made spontaneous?

Correct AnswerverifiedThe nonspontaneous process is coupled wi...View AnswerShow Answer

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 6 N2O(g) + 6 NO2(g) → 18 NO(g)

Correct AnswerverifiedShow Answer

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

Correct Answer
verified
Allotropes are diffe...
View Answer

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

Correct Answer
verified

Which of the following is NOT true for ΔG_rxn?

Correct Answer
verified

For the following example,identify the following. 2 F₂O(g) → 2 F₂(g) + O₂(g)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
Some of th...
View Answer

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 3 O₂(g) → 2 O₃(g) ΔG° = +326 kJ P(O₂) = 0.41 atm,P(O₃) = 5.2 atm

Correct Answer
verified

Place the following in order of decreasing molar entropy at 298 K. H₂ Cl₂ F₂

Correct Answer
verified

Correct Answer
verified
Entropy is a thermodynamic fun...
View Answer

Above what temperature does the following reaction become nonspontaneous? 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K

Correct Answer
verified

Calculate ΔS°_rxn for the following reaction.The S° for each species is shown below the reaction. N₂H₄(l) + H₂(g) → 2 NH₃(g) S° (J/mol∙K) 121.2 130.7 192.8

Correct Answer
verified

Estimate ΔG°_rxn for the following reaction at 449.0 K. CH₂O(g) + 2 H₂(g) → CH₄(g) + H₂O(g) ΔH°= -94.9 kJ; ΔS°= -224.2 J/K

Correct Answer
verified

Calculate ΔS°_rxn for the following reaction.The S° for each species is shown below the reaction. 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) S°(J/mol∙K) 192.8 205.2 210.8 188.8

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
The nonspontaneous process is coupled wi...
View Answer

Given the following equation, N₂O(g) + NO₂(g) → 3 NO(g) ΔG°_rxn = -23.0 kJ Calculate ΔG°_rxn for the following reaction. 6 N₂O(g) + 6 NO₂(g) → 18 NO(g)

Correct Answer
verified