Question 1

Given: H2O(l)   →\rightarrow→  H2O(s) ,  Δ\DeltaΔ H °\degree°  = -6.02 kJ at 273K, calculate the entropy change of the surroundings ( Δ\DeltaΔ Ssurr)  when one mole of water freezes at 0 °\degree° C and a pressure of one atmosphere.

Accepted Answer

A)   22.1 J/K
B)   -22.1 J/K
C)   397 J/K
D)   -397 J/K
E)   0.022 J/K F) C) and D)
G) B) and E)

Question 2

Which relationship or statement best describes  Δ\DeltaΔ S °\degree°  for the following reaction? 2H2S(g)  + 3O2(g)   →\rightarrow→ 2H2O(g)  + 2SO2(g)

Accepted Answer

A)   ( Δ\DeltaΔ S °\degree°≈\approx≈  0) 
B)   ( Δ\DeltaΔ S °\degree°  
C)   ( Δ\DeltaΔ S °\degree°  > 0) 
D)   ( Δ\DeltaΔ S °\degree° =  Δ\DeltaΔ H °\degree° /T) 
E)   More information is needed to make a reasonable prediction. F) C) and E)
G) None of the above B

Question 3

A reaction has a positive value of $\Delta$H$\degree$  and a positive value of $\Delta$S$\degree$ . Draw a neat, labeled schematic plot to show how $\Delta$G$\degree$  (y-axis) will depend on absolute temperature (x-axis).

Accepted Answer

The answer of A reaction has a positive value of...

Question 4

In a spontaneous process, the entropy of the system always increases.

Accepted Answer

A) True 
 B)False  False

Question 5

For a chemical reaction to be spontaneous only at low temperatures, which of the following conditions must be met?

Accepted Answer

A)  (  Δ\DeltaΔ S °\degree°   > 0,  Δ\DeltaΔ H °\degree°  > 0) 
B)   ( Δ\DeltaΔ S °\degree°   > 0,  Δ\DeltaΔ H °\degree° 
C)   ( Δ\DeltaΔ S °\degree°   Δ\DeltaΔ H °\degree°  
D)   ( Δ\DeltaΔ S °\degree°   Δ\DeltaΔ H °\degree°  > 0) 
E)   ( Δ\DeltaΔ G °\degree°  > 0)  F) A) and E)
G) C) and D)

Question 6

You are given pure samples of ethane, C2H6(g) , and toluene, C7H8(l) . What prediction would you make concerning their standard molar entropies at 298 K?

Accepted Answer

A)   S °\degree° ethane > S °\degree° toluene
B)   S °\degree° ethane °\degree° toluene
C)   S °\degree° ethane  ≈\approx≈  (S °\degree° toluene)  / 3
D)   S °\degree° ethane  ≈\approx≈ S °\degree° toluene
E)   Since toluene is much more complex than ethane, but ethane is in the gas phase while toluene is a liquid, none of these predictions can be confidently made without further information or calculations. F) B) and E)
G) B) and D)

Question 7

Which of the following results in a decrease in the entropy of the system?

Accepted Answer

A)   O2(g) , 300 K  →\rightarrow→  O2(g) , 400 K
B)   H2O(s) , 0 °\degree° C  →\rightarrow→ H2O(l) , 0 °\degree° C
C)   N2(g) , 25 °\degree° C  →\rightarrow→  N2(aq) , 25 °\degree° C
D)   NH3(l) , -34.5 °\degree° C  →\rightarrow→ NH3(g) , -34.5 °\degree° C
E)   2H2O2(g)   →\rightarrow→  2H2O(g)  + O2(g)  F) None of the above
G) A) and B)

Question 8

Given: C2H2(g) $\rightarrow$ 2C(graphite) + H2(g), $\Delta$G$\degree$ = -209 kJ
A sample of gaseous C2H2 (acetylene, or ethyne) was stored for one year, yet at the end of this period, the sample remained unchanged and no graphite or hydrogen gas had been formed. Briefly explain why there is no inconsistency between the sign of $\Delta$G$\degree$ and the apparent stability of the sample.

Accepted Answer

Relative to graphite and hydrogen, acety...

Question 9

What is the free energy change,  Δ\DeltaΔ G °\degree°  , for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453 °\degree° C?
 Kc = 0.020 c = 0.020   A)  6.4 kJ B)  8.8 kJ C)  15 kJ D)  19 kJ E)  24 kJ " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   6.4 kJ
B)   8.8 kJ
C)   15 kJ
D)   19 kJ
E)   24 kJ F) A) and E)
G) B) and E)

Question 10

A reaction has  Δ\DeltaΔ G= 10.0 kJ and  Δ\DeltaΔ G °\degree°  = 15.0 kJ at a temperature of 50 °\degree° C. Calculate the value of the reaction quotient Q under these conditions.

Accepted Answer

A)   0.16
B)   9.1 * 10¯5
C)   1.1 *104
D)   6.4
E)   6.0 * 10¯6 F) C) and D)
G) A) and B)

Question 11

Calculate Δ\DeltaΔ S  °\degree° for the reaction

Accepted Answer

A)   -254.96 J/K
B)   -198.02 J/K
C)   198.02 J/K
D)   254.96 J/K
E)   471.86 J/K F) B) and D)
G) C) and D)

Question 12

Which relationship or statement best describes  Δ\DeltaΔ S °\degree°  for the following reaction?
 Pb(s)  + Cl2(g)   →\rightarrow→  PbCl2(s)

Accepted Answer

A)   ( Δ\DeltaΔ S °\degree°   ≈\approx≈  0) 
B)  (  Δ\DeltaΔ S °\degree°  
C)   ( Δ\DeltaΔ S °\degree°  > 0) 
D)  (  Δ\DeltaΔ S °\degree°  =  Δ\DeltaΔ H °\degree° /T) 
E)   More information is needed to make a reasonable prediction. F) A) and B)
G) C) and D)

Question 13

The reaction of methane with water to form carbon dioxide and hydrogen is non-spontaneous at 298 K. At what temperature will this system make the transition from non-spontaneous to spontaneous? The data refer to 298 K.

Accepted Answer

A)   658 K
B)   683 K
C)   955 K
D)   1047 K
E)   1229 KF) A) and E)
G) All of the above

Question 14

For any reaction, if $\Delta$G $\degree$ > 0, then K < 1.

Accepted Answer

A) True 
 B)False

Question 15

A reaction is proceeding towards equilibrium. At a certain stage, the concentrations of reactants and products are such that  Δ\DeltaΔ G  =  Δ\DeltaΔ G °\degree°  . What conclusion can reasonably be drawn about the reaction at this time?

Accepted Answer

A)   K > Q
B)   K 
C)   K = Q
D)   K = 1
E)   Q = 1 F) A) and B)
G) B) and E)

Question 16

In tables of thermodynamic data provided in chemistry books, one finds $\Delta$H$\degree$ S1U1B1fS1U1B0, $\Delta$G$\degree$ S1U1B1fS1U1B0 and S$\degree$listed. Briefly, explain why the entropy data are supplied as S$\degree$, while the enthalpy and free energy data are in the form of $\Delta$H$\degree$ S1U1B1fS1U1B0 and $\Delta$G$\degree$ 1U1B1fS1U1B0, respectively.

Accepted Answer

The third law specifies the state of zer...

Question 17

You are given pure samples of ammonia, NH3(g) , and nitrogen trifluoride, NF3(g) . What prediction would you make concerning their standard molar entropies at 298 K?

Accepted Answer

A)   S °\degree° ammonia > S °\degree° nitrogen trifluoride
B)   S °\degree° ammonia °\degree° nitrogen trifluoride
C)   S °\degree° ammonia  ≈\approx≈  S °\degree° nitrogen trifluoride
D)   Other conditions need to be specified before a reliable prediction can be made.
E)   Even if more conditions are specified, a reliable prediction cannot be made. F) A) and C)
G) A) and B)

Question 18

Which, if any, of the following processes is spontaneous under the specified conditions?

Accepted Answer

A)   H2O(l)   →\rightarrow→  H2O(s)  at 25 °\degree° C
B)   CO2(s)   →\rightarrow→  CO2(g)  at 0 °\degree° C
C)   2H2O(g)   →\rightarrow→ H2(g)  + O2(g) 
D)   C(graphite)   →\rightarrow→  C(diamond)  at 25 °\degree° C and 1 atm pressure
E)   None of these choices is spontaneous. F) D) and E)
G) C) and E) B

Question 19

The free energy of a perfect crystal at absolute zero, is zero.

Accepted Answer

A) True 
 B)False

Question 20

Calculate  Δ\DeltaΔ G °\degree° for the combustion of propane.

Accepted Answer

A)   -2073.1 kJ
B)   -1387.3 kJ
C)   -598.5 kJ
D)   598.5 kJ
E)   2073.1 kJ F) A) and B)
G) B) and C)

Exam 20: Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Given: H₂O(l) $\rightarrow$ H₂O(s) , $\Delta$ H $\degree$ = -6.02 kJ at 273K, calculate the entropy change of the surroundings ( $\Delta$ S_surr) when one mole of water freezes at 0 $\degree$ C and a pressure of one atmosphere.

Correct Answer
verified

Which relationship or statement best describes $\Delta$ S $\degree$ for the following reaction? 2H₂S(g) + 3O₂(g) $\rightarrow$ 2H₂O(g) + 2SO₂(g)

Correct Answer
verified
B

A reaction has a positive value of $\Delta$ H $\degree$ and a positive value of $\Delta$ S $\degree$ . Draw a neat, labeled schematic plot to show how $\Delta$ G $\degree$ (y-axis) will depend on absolute temperature (x-axis).

Correct Answer
verified

In a spontaneous process, the entropy of the system always increases.

Correct Answer
verified
False

For a chemical reaction to be spontaneous only at low temperatures, which of the following conditions must be met?

Correct Answer
verified

You are given pure samples of ethane, C₂H₆(g) , and toluene, C₇H₈(l) . What prediction would you make concerning their standard molar entropies at 298 K?

Correct Answer
verified

Which of the following results in a decrease in the entropy of the system?

Correct Answer
verified

Correct Answer
verified
Relative to graphite and hydrogen, acety...
View Answer

Correct Answer
verified

A reaction has $\Delta$ G= 10.0 kJ and $\Delta$ G $\degree$ = 15.0 kJ at a temperature of 50 $\degree$ C. Calculate the value of the reaction quotient Q under these conditions.

Correct Answer
verified

Calculate $\Delta$ S $\degree$ for the reaction $Calculate \Delta S \degree for the reaction A) -254.96 J/K B) -198.02 J/K C) 198.02 J/K D) 254.96 J/K E) 471.86 J/K$ $Calculate \Delta S \degree for the reaction A) -254.96 J/K B) -198.02 J/K C) 198.02 J/K D) 254.96 J/K E) 471.86 J/K$

Correct Answer
verified

Which relationship or statement best describes $\Delta$ S $\degree$ for the following reaction? Pb(s) + Cl₂(g) $\rightarrow$ PbCl₂(s)

Correct Answer
verified

The reaction of methane with water to form carbon dioxide and hydrogen is non-spontaneous at 298 K. At what temperature will this system make the transition from non-spontaneous to spontaneous? The data refer to 298 K.

Correct Answer
verified

For any reaction, if $\Delta$ G $\degree$ > 0, then K < 1.

Correct Answer
verified

A reaction is proceeding towards equilibrium. At a certain stage, the concentrations of reactants and products are such that $\Delta$ G = $\Delta$ G $\degree$ . What conclusion can reasonably be drawn about the reaction at this time?

Correct Answer
verified

Correct Answer
verified
The third law specifies the state of zer...
View Answer

You are given pure samples of ammonia, NH₃(g) , and nitrogen trifluoride, NF₃(g) . What prediction would you make concerning their standard molar entropies at 298 K?

Correct Answer
verified

Which, if any, of the following processes is spontaneous under the specified conditions?

Correct Answer
verified
B

The free energy of a perfect crystal at absolute zero, is zero.

Correct Answer
verified

Correct Answer
verified

Exam 20: Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Given: H2O(l) →\rightarrow→ H2O(s) , Δ\DeltaΔ H °\degree° = -6.02 kJ at 273K, calculate the entropy change of the surroundings ( Δ\DeltaΔ Ssurr) when one mole of water freezes at 0 °\degree° C and a pressure of one atmosphere.

Correct AnswerverifiedShow Answer

Which relationship or statement best describes Δ\DeltaΔ S °\degree° for the following reaction? 2H2S(g) + 3O2(g) →\rightarrow→ 2H2O(g) + 2SO2(g)

Correct AnswerverifiedB

A reaction has a positive value of Δ\DeltaΔ H °\degree° and a positive value of Δ\DeltaΔ S °\degree° . Draw a neat, labeled schematic plot to show how Δ\DeltaΔ G °\degree° (y-axis) will depend on absolute temperature (x-axis).

Correct AnswerverifiedShow Answer

In a spontaneous process, the entropy of the system always increases.

Correct AnswerverifiedFalse

For a chemical reaction to be spontaneous only at low temperatures, which of the following conditions must be met?

Correct AnswerverifiedShow Answer

You are given pure samples of ethane, C2H6(g) , and toluene, C7H8(l) . What prediction would you make concerning their standard molar entropies at 298 K?

Correct AnswerverifiedShow Answer

Which of the following results in a decrease in the entropy of the system?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedRelative to graphite and hydrogen, acety...View AnswerShow Answer

What is the free energy change, Δ\DeltaΔ G °\degree° , for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453 °\degree° C? Kc = 0.020

Correct AnswerverifiedShow Answer

A reaction has Δ\DeltaΔ G= 10.0 kJ and Δ\DeltaΔ G °\degree° = 15.0 kJ at a temperature of 50 °\degree° C. Calculate the value of the reaction quotient Q under these conditions.

Correct AnswerverifiedShow Answer

Calculate Δ\DeltaΔ S °\degree° for the reaction

Correct AnswerverifiedShow Answer

Which relationship or statement best describes Δ\DeltaΔ S °\degree° for the following reaction? Pb(s) + Cl2(g) →\rightarrow→ PbCl2(s)

Correct AnswerverifiedShow Answer

The reaction of methane with water to form carbon dioxide and hydrogen is non-spontaneous at 298 K. At what temperature will this system make the transition from non-spontaneous to spontaneous? The data refer to 298 K.

Correct AnswerverifiedShow Answer

For any reaction, if Δ\DeltaΔ G °\degree° > 0, then K < 1.

Correct AnswerverifiedShow Answer

A reaction is proceeding towards equilibrium. At a certain stage, the concentrations of reactants and products are such that Δ\DeltaΔ G = Δ\DeltaΔ G °\degree° . What conclusion can reasonably be drawn about the reaction at this time?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedThe third law specifies the state of zer...View AnswerShow Answer

You are given pure samples of ammonia, NH3(g) , and nitrogen trifluoride, NF3(g) . What prediction would you make concerning their standard molar entropies at 298 K?

Correct AnswerverifiedShow Answer

Which, if any, of the following processes is spontaneous under the specified conditions?

Correct AnswerverifiedB

The free energy of a perfect crystal at absolute zero, is zero.

Correct AnswerverifiedShow Answer

Calculate Δ\DeltaΔ G °\degree° for the combustion of propane.

Correct AnswerverifiedShow Answer

Given: H₂O(l) $\rightarrow$ H₂O(s) , $\Delta$ H $\degree$ = -6.02 kJ at 273K, calculate the entropy change of the surroundings ( $\Delta$ S_surr) when one mole of water freezes at 0 $\degree$ C and a pressure of one atmosphere.

Correct Answer
verified

Which relationship or statement best describes $\Delta$ S $\degree$ for the following reaction? 2H₂S(g) + 3O₂(g) $\rightarrow$ 2H₂O(g) + 2SO₂(g)

Correct Answer
verified
B

A reaction has a positive value of $\Delta$ H $\degree$ and a positive value of $\Delta$ S $\degree$ . Draw a neat, labeled schematic plot to show how $\Delta$ G $\degree$ (y-axis) will depend on absolute temperature (x-axis).

Correct Answer
verified

Correct Answer
verified
False

Correct Answer
verified

You are given pure samples of ethane, C₂H₆(g) , and toluene, C₇H₈(l) . What prediction would you make concerning their standard molar entropies at 298 K?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
Relative to graphite and hydrogen, acety...
View Answer

Correct Answer
verified

A reaction has $\Delta$ G= 10.0 kJ and $\Delta$ G $\degree$ = 15.0 kJ at a temperature of 50 $\degree$ C. Calculate the value of the reaction quotient Q under these conditions.

Correct Answer
verified

Calculate $\Delta$ S $\degree$ for the reaction $Calculate \Delta S \degree for the reaction A) -254.96 J/K B) -198.02 J/K C) 198.02 J/K D) 254.96 J/K E) 471.86 J/K$ $Calculate \Delta S \degree for the reaction A) -254.96 J/K B) -198.02 J/K C) 198.02 J/K D) 254.96 J/K E) 471.86 J/K$

Correct Answer
verified

Which relationship or statement best describes $\Delta$ S $\degree$ for the following reaction? Pb(s) + Cl₂(g) $\rightarrow$ PbCl₂(s)

Correct Answer
verified

Correct Answer
verified

For any reaction, if $\Delta$ G $\degree$ > 0, then K < 1.

Correct Answer
verified

A reaction is proceeding towards equilibrium. At a certain stage, the concentrations of reactants and products are such that $\Delta$ G = $\Delta$ G $\degree$ . What conclusion can reasonably be drawn about the reaction at this time?

Correct Answer
verified

Correct Answer
verified
The third law specifies the state of zer...
View Answer

You are given pure samples of ammonia, NH₃(g) , and nitrogen trifluoride, NF₃(g) . What prediction would you make concerning their standard molar entropies at 298 K?

Correct Answer
verified

Correct Answer
verified
B

Correct Answer
verified

Correct Answer
verified