Calculate the standard entropy change for the following reaction: 2 SO2(g)+ O2(g)→ 2 SO3(g) Given: S°[SO2(g)] = 248.2 J/K⋅mol,S°[O2(g)] = 205.1 J/K⋅mol,and S°[SO3(g)] = 256.8 J/K⋅mol.

A) -196.5 J/K·mol-rxn B) -94.0 J/K·mol-rxn C) -187.9 J/K·mol-rxn D) +187.9 J/K·mol-rxn E) +196.5 J/K·mol-rxn A) -196.5 J/K·mol-rxn B) -94.0 J/K·mol-rxn C) -187.9 J/K·mol-rxn D) +187.9 J/K·mol-rxn E) +196.5 J/K·mol-rxn

Calculate ΔrG° for the reaction below at 25.0 °C. CH4(g)+ H2O(g)→ 3 H2(g)+ CO(g) Given: ΔfG° [CH4(g)] = -50.8 kJ/mol,ΔfG° [H2O(g)] = -228.6 kJ/mol,ΔfG° [H2(g)] = 0.0 kJ/mol,and ΔfG° [CO(g)] = -137.2 kJ/mol.

A) -416.3 kJ/mol-rxn B) -142.2 kJ/mol-rxn C) +142.2 kJ/mol-rxn D) +315.0 kJ/mol-rxn E) +416.3 kJ/mol-rxn A) -416.3 kJ/mol-rxn B) -142.2 kJ/mol-rxn C) +142.2 kJ/mol-rxn D) +315.0 kJ/mol-rxn E) +416.3 kJ/mol-rxn

Hydrogen gas is prepared by electrolysis of water according to the reaction below. 2 H2O( )→ 2 H2(g)+ O2(g) Predict the signs of ΔrH and ΔrS.

A) ΔrH > 0 and ΔrS > 0 B) ΔrH rS > 0 C) ΔrH > 0 and ΔrS rH rS rH = 0 and ΔrS 0 and ΔrS > 0 B) ΔrH rS > 0 C) ΔrH > 0 and ΔrS rH rS rH = 0 and ΔrS < 0

Given the following data: S(g)+ O2(g)→ SO2(g) ΔrG° = -300.1 kJ/mol-rxn 2 S(g)+ 3 O2(g)→ 2 SO3(g) ΔrG° = -742.1 kJ/mol-rxn Calculate ΔfG° for the reaction below. SO2(g)+ 1/2 O2(g)→ SO3(g)

A) -1042.2 kJ/mol-rxn B) -71.0 kJ/mol-rxn C) +2.47 kJ/mol-rxn D) +71.0 kJ/mol-rxn E) +1042.2 kJ/mol-rxn A) -1042.2 kJ/mol-rxn B) -71.0 kJ/mol-rxn C) +2.47 kJ/mol-rxn D) +71.0 kJ/mol-rxn E) +1042.2 kJ/mol-rxn

The Ksp of silver bromide is 5.4 × 10−13 at 298 K. AgBr(s) Ag+(aq)+ Br−(aq) What is ΔrG°? (R = 8.314 J/K⋅mol)

A) −3.0 × 101 kJ/mol B) −5.87 kJ/mol C) 5.87 kJ/mol D) 3.0 × 101 kJ/mol E) 7.0 × 101 kJ/mol A) −3.0 × 101 kJ/mol B) −5.87 kJ/mol C) 5.87 kJ/mol D) 3.0 × 101 kJ/mol E) 7.0 × 101 kJ/mol

What is the standard entropy change for the following reaction? 4 N2(g) + 12 H2(g) → 8 NH3(g) (J/mol⋅K) 191)5 130)6 192)3

A) -794.8 J/K⋅mol-rxn B) 794.8 J/K⋅mol-rxn C) 2948.8 J/K⋅mol-rxn D) -2948.8 J/K⋅mol-rxn E) -129.8 J/K⋅mol-rxn A) -794.8 J/K⋅mol-rxn B) 794.8 J/K⋅mol-rxn C) 2948.8 J/K⋅mol-rxn D) -2948.8 J/K⋅mol-rxn E) -129.8 J/K⋅mol-rxn

Exam 19: Principles of Chemical Reactivity: Entropy and Free Energy

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Does the formation of complex molecules such as proteins and nucleic acids from more simple molecules contradict the second law of thermodynamics?

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Question 21

Calculate the standard entropy change for the following reaction: 2 SO₂(g)+ O₂(g)→ 2 SO₃(g) Given: S°[SO₂(g)] = 248.2 J/K⋅mol,S°[O₂(g)] = 205.1 J/K⋅mol,and S°[SO₃(g)] = 256.8 J/K⋅mol.

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Question 22

A change of state occurring in a system is accompanied by 60.7 kJ of heat that is transferred to the surroundings at a constant pressure and at a constant temperature of 300 K.Calculate the ΔS(surroundings)for the process.

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Question 23

Calculate Δ_rG° for the reaction below at 25.0 °C. CH₄(g)+ H₂O(g)→ 3 H₂(g)+ CO(g) Given: Δ_fG° [CH₄(g)] = -50.8 kJ/mol,Δ_fG° [H₂O(g)] = -228.6 kJ/mol,Δ_fG° [H₂(g)] = 0.0 kJ/mol,and Δ_fG° [CO(g)] = -137.2 kJ/mol.

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Question 24

If a cube of ice at 0 °C is placed outside on a warm summer day,the ice will melt spontaneously.What are the signs of Δ_rH,Δ_rS,and Δ_rG for the process?

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Question 25

In which of the following reactions is Δ_rS° expected to be positive?

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Question 26

Hydrogen gas is prepared by electrolysis of water according to the reaction below. 2 H₂O( )→ 2 H₂(g)+ O₂(g) Predict the signs of Δ_rH and Δ_rS.

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Question 27

Given the following data: S(g)+ O₂(g)→ SO₂(g) Δ_rG° = -300.1 kJ/mol-rxn 2 S(g)+ 3 O₂(g)→ 2 SO₃(g) Δ_rG° = -742.1 kJ/mol-rxn Calculate Δ_fG° for the reaction below. SO₂(g)+ 1/2 O₂(g)→ SO₃(g)

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Question 28

The standard entropy for the formation of sulfur hexafluoride from the sulfur and fluorine is -348.7 J/K ⋅mol-rxn at 298.15 K.What is the standard molar entropy of sulfur hexafluoride for the reaction below? (Given: S°[S(s)] = 32.1 J/K ⋅mol and S°[F2(g)] = 202.8 J/K ⋅mol)

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Question 29

The K_spof silver bromide is 5.4 × 10−¹³ at 298 K. AgBr(s) Ag⁺(aq)+ Br−(aq) What is Δ_rG°? (R = 8.314 J/K⋅mol)

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Question 30

_____ changes only occur in the direction that leads toward chemical equilibrium.

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Question 31

The standard free energy change for a chemical reaction is +13.3 kJ/mol.Which of the following is the equilibrium constant for the reaction at 125 °C? (R = 8.314 J/K⋅mol)

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Question 32

When a real gas is compressed from low pressure to high pressure,its temperature increases.Which of the following is true for ΔH and ΔS?

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Question 33

For any process,the change in entropy of the universe equals the sum of the entropy changes for the system and for the ________.

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Question 34

What is the S0 for ozone if the standard entropy change for the reaction below is 411 J/K⋅mol-rxn and S⁰[O₂(g)] = 205 J/K⋅mol. 6 O₃(g)→ 9 O₂(g)

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Question 35

What is the standard entropy change for the following reaction? 4 N₂(g) + 12 H₂(g) → 8 NH₃(g) (J/mol⋅K) 191)5 130)6 192)3

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Question 36

A 100 mL sample of water is placed in a coffee cup calorimeter.When 1.0 g of an ionic solid is added,the temperature decreases from 21.5 °C to 20.8 °C as the solid dissolves.For the dissolving of the solid,_____.

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Question 37

For a chemical reaction,if Δ_rG° = 0,then _____.

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Question 38

If Δ_rG° > 0 for a reaction at all temperatures,then Δ_rH° is _____ and Δ_rS° is _____.

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Question 39

The change in entropy for any process is not dependent upon the pathway by which the process occurs.In other words,the change in entropy for any process is a(n)_____ function.

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Question 40

Showing 21 - 40 of 66

Exam 19: Principles of Chemical Reactivity: Entropy and Free Energy

Does the formation of complex molecules such as proteins and nucleic acids from more simple molecules contradict the second law of thermodynamics?

Calculate the standard entropy change for the following reaction: 2 SO2(g)+ O2(g)→ 2 SO3(g) Given: S°[SO2(g)] = 248.2 J/K⋅mol,S°[O2(g)] = 205.1 J/K⋅mol,and S°[SO3(g)] = 256.8 J/K⋅mol.

A change of state occurring in a system is accompanied by 60.7 kJ of heat that is transferred to the surroundings at a constant pressure and at a constant temperature of 300 K.Calculate the ΔS(surroundings)for the process.

Calculate ΔrG° for the reaction below at 25.0 °C. CH4(g)+ H2O(g)→ 3 H2(g)+ CO(g) Given: ΔfG° [CH4(g)] = -50.8 kJ/mol,ΔfG° [H2O(g)] = -228.6 kJ/mol,ΔfG° [H2(g)] = 0.0 kJ/mol,and ΔfG° [CO(g)] = -137.2 kJ/mol.

If a cube of ice at 0 °C is placed outside on a warm summer day,the ice will melt spontaneously.What are the signs of ΔrH,ΔrS,and ΔrG for the process?

In which of the following reactions is ΔrS° expected to be positive?

Hydrogen gas is prepared by electrolysis of water according to the reaction below. 2 H2O( )→ 2 H2(g)+ O2(g) Predict the signs of ΔrH and ΔrS.

Given the following data: S(g)+ O2(g)→ SO2(g) ΔrG° = -300.1 kJ/mol-rxn 2 S(g)+ 3 O2(g)→ 2 SO3(g) ΔrG° = -742.1 kJ/mol-rxn Calculate ΔfG° for the reaction below. SO2(g)+ 1/2 O2(g)→ SO3(g)

The standard entropy for the formation of sulfur hexafluoride from the sulfur and fluorine is -348.7 J/K ⋅mol-rxn at 298.15 K.What is the standard molar entropy of sulfur hexafluoride for the reaction below? (Given: S°[S(s)] = 32.1 J/K ⋅mol and S°[F2(g)] = 202.8 J/K ⋅mol)

The Ksp of silver bromide is 5.4 × 10−13 at 298 K. AgBr(s) Ag+(aq)+ Br−(aq) What is ΔrG°? (R = 8.314 J/K⋅mol)

_____ changes only occur in the direction that leads toward chemical equilibrium.

The standard free energy change for a chemical reaction is +13.3 kJ/mol.Which of the following is the equilibrium constant for the reaction at 125 °C? (R = 8.314 J/K⋅mol)

When a real gas is compressed from low pressure to high pressure,its temperature increases.Which of the following is true for ΔH and ΔS?

For any process,the change in entropy of the universe equals the sum of the entropy changes for the system and for the ________.

What is the S0 for ozone if the standard entropy change for the reaction below is 411 J/K⋅mol-rxn and S0[O2(g)] = 205 J/K⋅mol. 6 O3(g)→ 9 O2(g)

What is the standard entropy change for the following reaction? 4 N2(g) + 12 H2(g) → 8 NH3(g) (J/mol⋅K) 191)5 130)6 192)3

A 100 mL sample of water is placed in a coffee cup calorimeter.When 1.0 g of an ionic solid is added,the temperature decreases from 21.5 °C to 20.8 °C as the solid dissolves.For the dissolving of the solid,_____.

For a chemical reaction,if ΔrG° = 0,then _____.

If ΔrG° > 0 for a reaction at all temperatures,then ΔrH° is _____ and ΔrS° is _____.

The change in entropy for any process is not dependent upon the pathway by which the process occurs.In other words,the change in entropy for any process is a(n)_____ function.

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Chemical Kinetics: the Rates of Chemical Reactions

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Calculate the standard entropy change for the following reaction: 2 SO₂(g)+ O₂(g)→ 2 SO₃(g) Given: S°[SO₂(g)] = 248.2 J/K⋅mol,S°[O₂(g)] = 205.1 J/K⋅mol,and S°[SO₃(g)] = 256.8 J/K⋅mol.

Calculate Δ_rG° for the reaction below at 25.0 °C. CH₄(g)+ H₂O(g)→ 3 H₂(g)+ CO(g) Given: Δ_fG° [CH₄(g)] = -50.8 kJ/mol,Δ_fG° [H₂O(g)] = -228.6 kJ/mol,Δ_fG° [H₂(g)] = 0.0 kJ/mol,and Δ_fG° [CO(g)] = -137.2 kJ/mol.

If a cube of ice at 0 °C is placed outside on a warm summer day,the ice will melt spontaneously.What are the signs of Δ_rH,Δ_rS,and Δ_rG for the process?

In which of the following reactions is Δ_rS° expected to be positive?

Hydrogen gas is prepared by electrolysis of water according to the reaction below. 2 H₂O( )→ 2 H₂(g)+ O₂(g) Predict the signs of Δ_rH and Δ_rS.

Given the following data: S(g)+ O₂(g)→ SO₂(g) Δ_rG° = -300.1 kJ/mol-rxn 2 S(g)+ 3 O₂(g)→ 2 SO₃(g) Δ_rG° = -742.1 kJ/mol-rxn Calculate Δ_fG° for the reaction below. SO₂(g)+ 1/2 O₂(g)→ SO₃(g)

The K_spof silver bromide is 5.4 × 10−¹³ at 298 K. AgBr(s) Ag⁺(aq)+ Br−(aq) What is Δ_rG°? (R = 8.314 J/K⋅mol)

What is the S0 for ozone if the standard entropy change for the reaction below is 411 J/K⋅mol-rxn and S⁰[O₂(g)] = 205 J/K⋅mol. 6 O₃(g)→ 9 O₂(g)

What is the standard entropy change for the following reaction? 4 N₂(g) + 12 H₂(g) → 8 NH₃(g) (J/mol⋅K) 191)5 130)6 192)3

For a chemical reaction,if Δ_rG° = 0,then _____.

If Δ_rG° > 0 for a reaction at all temperatures,then Δ_rH° is _____ and Δ_rS° is _____.