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.

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 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

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

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

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

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 ) 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 )

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

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 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

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.

(Multiple Choice)

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Question 41

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

(True/False)

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Question 42

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.

(Essay)

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Question 43

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

(Multiple Choice)

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Question 44

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.

(Short Answer)

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Question 45

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.

(True/False)

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Question 46

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

(Short Answer)

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Question 47

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.

(Multiple Choice)

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Question 48

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

(Multiple Choice)

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Question 49

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

(Multiple Choice)

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Question 50

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

(Multiple Choice)

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Question 51

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

(Multiple Choice)

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Question 52

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

(Multiple Choice)

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Question 53

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.

(Multiple Choice)

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Question 54

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

(Multiple Choice)

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Question 55

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

(Multiple Choice)

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Question 56

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

(Short Answer)

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Question 57

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?

(Essay)

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Question 58

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.

(Multiple Choice)

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Question 59

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

(True/False)

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Question 60

Showing 41 - 60 of 95

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.

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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.

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Physical Equilibria

Chemical Equilibria

Acids and Bases

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

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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.