Question 1

Use the Boltzmann formula to calculate the entropy at T = 0 of 1.00 mol chlorobenzene,C6H5Cl,where each molecule can be oriented in any of six ways.

Accepted Answer

A) 0 J.K-1; at T = 0,there is no randomness. 
B) (-15 J.K-1) 
C) (-30 J.K-1) 
D) +30 J.K-1 
E) +15 J.K-1

Question 2

The entropy of vaporization of a substance is always larger than its entropy of fusion.

Accepted Answer

A) True 
 B)False

Question 3

The hydrolysis of ATP to ADP is spontaneous.However,the reaction of glucose with monohydrogen phosphate,the first step in the oxidation of glucose,is not spontaneous.Determine whether the coupled reactions are spontaneous.

Accepted Answer

The answer of The hydrolysis of ATP to ADP is...

Question 4

For the reaction 
2SO3(g)$\rightarrow$2SO2(g)+ O2(g)
$\Delta$Hr° = +198 kJ.mol-1 and $\Delta$Sr° = 190 J.K-1.mol-1 at 298 K.The equilibrium constant for this reaction will be greater than 1 at

Accepted Answer

A) all temperatures. 
B) temperatures above 1315 K. 
C) temperatures below 1042 K. 
D) no temperature. 
E) temperatures above 1042 K.

Question 5

Use tabulated thermodynamic data to calculate the concentration of CO₂(aq)in equilibrium with an external pressure of 2.50 atm CO₂(g)at 298 K.

Accepted Answer

The answer of Use tabulated thermodynamic data to calculate the...

Question 6

The experimental value of the molar entropy of 1 mol NO at 0 K is about 5 J∙K-1.We can conclude that in the crystal the molecules of NO are arranged randomly.

Accepted Answer

A) True 
 B)False

Question 7

For He(g,10 atm)$\rightarrow$ He(g,1 atm),is the entropy change positive or negative?

Accepted Answer

The answer of For He(g,10 atm)$\rightarrow$ He(g,1 atm),is the entropy...

Question 8

Calculate the standard entropy of condensation of chloroform at its boiling point,335 K.The standard molar enthalpy of vaporization of chloroform at its boiling point is 31.4 J.K-1.mol-1 .

Accepted Answer

A) (-31.3 J.K-1.mol-1 ) 
B) +93.7 J.K-1.mol-1  
C) (-93.7 J.K-1.mol-1 ) 
D) +31.4 J.K-1.mol-1  
E) +506 J.K-1.mol-1

Question 9

Consider the following compounds and their standard free energies of formation:  Which of these liquids is (are)thermodynamically stable?

Accepted Answer

A) 2 and 4 
B) 2 and 3 
C) 1,3,and 5 
D) 1 
E) 3

Question 10

Consider the following compounds and their standard free energies of formation:  Which of these liquids is (are)thermodynamically unstable?

Accepted Answer

A) 2 
B) 1,3,and 5 
C) 1 and 4 
D) 2 and 3 
E) 2 and 4

Question 11

For the reaction 
2C(s)+ 2H2(g)$\rightarrow$C2H4(g)
$\Delta$HrS1U1P1$\circ$S1S1P0 = +52.3 kJ.mol-1 and $\Delta$SrS1U1P1$\circ$S1S1P0 = -53.07 J.K-1.mol-1 at 298 K.The reverse reaction will be spontaneous at

Accepted Answer

A) temperatures below 985 K. 
B) temperatures above 985 K. 
C) temperatures below 1015 K. 
D) all temperatures. 
E) no temperatures.

Question 12

Calculate $\Delta$Ssurr° at 298 K for the reaction 6C(s)+ 3H2(g)$\rightarrow$ C6H6(l)
$\Delta$Hr° = +49.0 J.K-1.mol-1 ,$\Delta$Sr° = -253 J.K-1.mol-1

Accepted Answer

A) +164 J.K-1.mol-1  
B) (-417 J.K-1.mol-1 ) 
C) +253 J.K-1.mol-1  
D) (-164 J.K-1.mol-1 ) 
E) (-253 J.K-1.mol-1 )

Question 13

Use Trouton's constant to estimate the enthalpy of vaporization of diethyl ether,which boils at 309 K.

Accepted Answer

A) +85 kJ.mol-1  
B) +26  kJ.mol-1  
C) +275  kJ.mol-1  
D) (-85  kJ.mol-1 ) 
E) +3.6  kJ.mol-1

Question 14

Calculate the standard entropy of vaporization of ethanol at its boiling point,352 K.The standard molar enthalpy of vaporization of ethanol at its boiling point is 40.5 J.K-1.mol-1 .

Accepted Answer

A) +40.5 J.K-1.mol-1  
B) +115 J.K-1.mol-1  
C) (-40.5 J.K-1.mol-1 ) 
D) +513 J.K-1.mol-1  
E) (-115 J.K-1.mol-1 )

Question 15

Consider the reaction Cl2(g)$\rightarrow$  2Cl(g)
Which of the following statement regarding this reaction is true?

Accepted Answer

A) The reaction is spontaneous at high temperatures. 
B) The reaction is spontaneous at low temperatures. 
C) The reaction is not spontaneous at any temperature. 
D) The reaction is spontaneous at all temperatures.

Question 16

The entropy of fusion of water is +22.0 J.K-1.mol-1  and the enthalpy of fusion of water is +6.01 J.K-1.mol-1   at 0S1U1P1$\circ$S1S1P0C.At 0S1U1P1$\circ$S1S1P0C,$\Delta$Stotal for the melting of ice is

Accepted Answer

A) (-6010 J.K-1.mol-1  ) 
B) 0. 
C) (-22.0 J.K-1.mol-1  ) 
D) +6010 J.K-1.mol-1  
E) +22.0 J.K-1.mol-1

Question 17

Calculate $\Delta$G for the process
He(g,1 atm,298 K)$\rightarrow$ He(g,10 atm,298 K)

Accepted Answer

The answer of Calculate $\Delta$G for the process
He(g,1 atm,298 K)$\rightarrow$...

Question 18

Draw a graph of the molar Gibbs free energy versus temperature for H₂O(l)and H₂O(g). (a)Explain the slopes of the 2 lines. (b)At low temperatures,which phase is most stable? (c)At high temperatures,which phase is more stable?

Accepted Answer

The answer of Draw a graph of the molar Gibbs...

Question 19

Calculate $\Delta$Stotal for the isothermal irreversible free expansion of 1.00 mol of ideal gas from 8.00 L to 20.00 L at 298 K.

Accepted Answer

A) 0 
B) +15.2 J.K-1.mol-1  
C) +7.6 J.K-1.mol-1  
D) (-15.2 J.K-1.mol-1 ) 
E) (-7.6 J.K-1.mol-1 )

Question 20

The change in molar entropy for vaporization of all liquids is about the same.

Accepted Answer

A) True 
 B)False

Exam 9: Thermodynamics: The Second and Third Laws

Use the Boltzmann formula to calculate the entropy at T = 0 of 1.00 mol chlorobenzene,C₆H₅Cl,where each molecule can be oriented in any of six ways.

The entropy of vaporization of a substance is always larger than its entropy of fusion.

The hydrolysis of ATP to ADP is spontaneous.However,the reaction of glucose with monohydrogen phosphate,the first step in the oxidation of glucose,is not spontaneous.Determine whether the coupled reactions are spontaneous.

For the reaction 2SO₃(g) $\rightarrow$ 2SO₂(g) + O₂(g) $\Delta$ H_r° = +198 kJ.mol^-1 and $\Delta$ S_r° = 190 J.K^-1.mol^-1 at 298 K.The equilibrium constant for this reaction will be greater than 1 at

Use tabulated thermodynamic data to calculate the concentration of CO₂(aq)in equilibrium with an external pressure of 2.50 atm CO₂(g)at 298 K.

The experimental value of the molar entropy of 1 mol NO at 0 K is about 5 J∙K^-1.We can conclude that in the crystal the molecules of NO are arranged randomly.

For He(g,10 atm) $\rightarrow$ He(g,1 atm),is the entropy change positive or negative?

Calculate the standard entropy of condensation of chloroform at its boiling point,335 K.The standard molar enthalpy of vaporization of chloroform at its boiling point is 31.4 J.K^-1.mol^-1.

Consider the following compounds and their standard free energies of formation: Which of these liquids is (are) thermodynamically stable?

Consider the following compounds and their standard free energies of formation: Which of these liquids is (are) thermodynamically unstable?

For the reaction 2C(s) + 2H₂(g) $\rightarrow$ C₂H₄(g) $\Delta$ H_r^$\circ$ = +52.3 kJ.mol^-1 and $\Delta$ S_r^$\circ$ = -53.07 J.K^-1.mol^-1 at 298 K.The reverse reaction will be spontaneous at

Calculate $\Delta$ S_surr° at 298 K for the reaction 6C(s) + 3H₂(g) $\rightarrow$ C₆H₆(l) $\Delta$ H_r° = +49.0 J.K^-1.mol^-1, $\Delta$ S_r° = -253 J.K^-1.mol^-1

Use Trouton's constant to estimate the enthalpy of vaporization of diethyl ether,which boils at 309 K.

Calculate the standard entropy of vaporization of ethanol at its boiling point,352 K.The standard molar enthalpy of vaporization of ethanol at its boiling point is 40.5 J.K^-1.mol^-1.

Consider the reaction Cl₂(g) $\rightarrow$ 2Cl(g) Which of the following statement regarding this reaction is true?

The entropy of fusion of water is +22.0 J.K^-1.mol^-1 and the enthalpy of fusion of water is +6.01 J.K^-1.mol^-1 at 0^$\circ$C.At 0^$\circ$C, $\Delta$ S_total for the melting of ice is

Calculate $\Delta$ G for the process He(g,1 atm,298 K) $\rightarrow$ He(g,10 atm,298 K)

Draw a graph of the molar Gibbs free energy versus temperature for H₂O(l)and H₂O(g). (a)Explain the slopes of the 2 lines. (b)At low temperatures,which phase is most stable? (c)At high temperatures,which phase is more stable?

Calculate $\Delta$ S_total for the isothermal irreversible free expansion of 1.00 mol of ideal gas from 8.00 L to 20.00 L at 298 K.

The change in molar entropy for vaporization of all liquids is about the same.

Exam 9: Thermodynamics: The Second and Third Laws

Use the Boltzmann formula to calculate the entropy at T = 0 of 1.00 mol chlorobenzene,C6H5Cl,where each molecule can be oriented in any of six ways.

The entropy of vaporization of a substance is always larger than its entropy of fusion.

The hydrolysis of ATP to ADP is spontaneous.However,the reaction of glucose with monohydrogen phosphate,the first step in the oxidation of glucose,is not spontaneous.Determine whether the coupled reactions are spontaneous.

For the reaction 2SO3(g) →\rightarrow→ 2SO2(g) + O2(g) Δ\DeltaΔ Hr° = +198 kJ.mol-1 and Δ\DeltaΔ Sr° = 190 J.K-1.mol-1 at 298 K.The equilibrium constant for this reaction will be greater than 1 at

Use tabulated thermodynamic data to calculate the concentration of CO2(aq)in equilibrium with an external pressure of 2.50 atm CO2(g)at 298 K.

The experimental value of the molar entropy of 1 mol NO at 0 K is about 5 J∙K-1.We can conclude that in the crystal the molecules of NO are arranged randomly.

For He(g,10 atm) →\rightarrow→ He(g,1 atm),is the entropy change positive or negative?

Calculate the standard entropy of condensation of chloroform at its boiling point,335 K.The standard molar enthalpy of vaporization of chloroform at its boiling point is 31.4 J.K-1.mol-1 .

Consider the following compounds and their standard free energies of formation: Which of these liquids is (are) thermodynamically stable?

Consider the following compounds and their standard free energies of formation: Which of these liquids is (are) thermodynamically unstable?

For the reaction 2C(s) + 2H2(g) →\rightarrow→ C2H4(g) Δ\DeltaΔ Hr ∘\circ∘ = +52.3 kJ.mol-1 and Δ\DeltaΔ Sr ∘\circ∘ = -53.07 J.K-1.mol-1 at 298 K.The reverse reaction will be spontaneous at

Calculate Δ\DeltaΔ Ssurr° at 298 K for the reaction 6C(s) + 3H2(g) →\rightarrow→ C6H6(l) Δ\DeltaΔ Hr° = +49.0 J.K-1.mol-1 , Δ\DeltaΔ Sr° = -253 J.K-1.mol-1

Use Trouton's constant to estimate the enthalpy of vaporization of diethyl ether,which boils at 309 K.

Calculate the standard entropy of vaporization of ethanol at its boiling point,352 K.The standard molar enthalpy of vaporization of ethanol at its boiling point is 40.5 J.K-1.mol-1 .

Consider the reaction Cl2(g) →\rightarrow→ 2Cl(g) Which of the following statement regarding this reaction is true?

The entropy of fusion of water is +22.0 J.K-1.mol-1 and the enthalpy of fusion of water is +6.01 J.K-1.mol-1 at 0 ∘\circ∘ C.At 0 ∘\circ∘ C, Δ\DeltaΔ Stotal for the melting of ice is

Calculate Δ\DeltaΔ G for the process He(g,1 atm,298 K) →\rightarrow→ He(g,10 atm,298 K)

Draw a graph of the molar Gibbs free energy versus temperature for H2O(l)and H2O(g). (a)Explain the slopes of the 2 lines. (b)At low temperatures,which phase is most stable? (c)At high temperatures,which phase is more stable?

Calculate Δ\DeltaΔ Stotal for the isothermal irreversible free expansion of 1.00 mol of ideal gas from 8.00 L to 20.00 L at 298 K.

The change in molar entropy for vaporization of all liquids is about the same.

Use the Boltzmann formula to calculate the entropy at T = 0 of 1.00 mol chlorobenzene,C₆H₅Cl,where each molecule can be oriented in any of six ways.

For the reaction 2SO₃(g) $\rightarrow$ 2SO₂(g) + O₂(g) $\Delta$ H_r° = +198 kJ.mol^-1 and $\Delta$ S_r° = 190 J.K^-1.mol^-1 at 298 K.The equilibrium constant for this reaction will be greater than 1 at

Use tabulated thermodynamic data to calculate the concentration of CO₂(aq)in equilibrium with an external pressure of 2.50 atm CO₂(g)at 298 K.

The experimental value of the molar entropy of 1 mol NO at 0 K is about 5 J∙K^-1.We can conclude that in the crystal the molecules of NO are arranged randomly.

For He(g,10 atm) $\rightarrow$ He(g,1 atm),is the entropy change positive or negative?

Calculate the standard entropy of condensation of chloroform at its boiling point,335 K.The standard molar enthalpy of vaporization of chloroform at its boiling point is 31.4 J.K^-1.mol^-1.

For the reaction 2C(s) + 2H₂(g) $\rightarrow$ C₂H₄(g) $\Delta$ H_r^$\circ$ = +52.3 kJ.mol^-1 and $\Delta$ S_r^$\circ$ = -53.07 J.K^-1.mol^-1 at 298 K.The reverse reaction will be spontaneous at

Calculate $\Delta$ S_surr° at 298 K for the reaction 6C(s) + 3H₂(g) $\rightarrow$ C₆H₆(l) $\Delta$ H_r° = +49.0 J.K^-1.mol^-1, $\Delta$ S_r° = -253 J.K^-1.mol^-1

Calculate the standard entropy of vaporization of ethanol at its boiling point,352 K.The standard molar enthalpy of vaporization of ethanol at its boiling point is 40.5 J.K^-1.mol^-1.

Consider the reaction Cl₂(g) $\rightarrow$ 2Cl(g) Which of the following statement regarding this reaction is true?

The entropy of fusion of water is +22.0 J.K^-1.mol^-1 and the enthalpy of fusion of water is +6.01 J.K^-1.mol^-1 at 0^$\circ$C.At 0^$\circ$C, $\Delta$ S_total for the melting of ice is

Calculate $\Delta$ G for the process He(g,1 atm,298 K) $\rightarrow$ He(g,10 atm,298 K)

Draw a graph of the molar Gibbs free energy versus temperature for H₂O(l)and H₂O(g). (a)Explain the slopes of the 2 lines. (b)At low temperatures,which phase is most stable? (c)At high temperatures,which phase is more stable?

Calculate $\Delta$ S_total for the isothermal irreversible free expansion of 1.00 mol of ideal gas from 8.00 L to 20.00 L at 298 K.