Calculate $\Delta$S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s)$\rarr$ 2Pb(s)+ CO2(g)given these absolute entropies:

A) +198.8 J/K·mol B) +488.0 J/K·mol C) +353.6 J/K·mol D) -203.3 J/K·mol E) +203.3 J/K·mol A) +198.8 J/K·mol B) +488.0 J/K·mol C) +353.6 J/K·mol D) -203.3 J/K·mol E) +203.3 J/K·mol

Calculate the equilibrium constant for the decomposition of water 2H2O(l) 2H2(g)+ O2(g) At 25°C, given that $\Delta$G°f (H2O(l))= -237.2 kJ/mol.

A) 0.83 B) 6.3 × 10-84 C) 2.5 × 10-42 D) 1.6 × 1083 E) 4.7 × 105 A) 0.83 B) 6.3 × 10-84 C) 2.5 × 10-42 D) 1.6 × 1083 E) 4.7 × 105

For the reaction 2 SO2(g)+ O2(g)$\rarr$ 2 SO3(g), if initially P(SO2)= 1.2 atm, P(O2)= 1.8 atm, and P(SO3)= 2.1 atm, calculate $\Delta$G for this reaction at 25°C.The following data is valid at 25°C:

A) -140.0 kJ/mol B) -137.6 kJ/mol C) -138.7 kJ/mol D) 1,174.7 kJ/mol E) -141.3 kJ/mol A) -140.0 kJ/mol B) -137.6 kJ/mol C) -138.7 kJ/mol D) 1,174.7 kJ/mol E) -141.3 kJ/mol

Arrange these reactions according to increasing $\Delta$S. 1)H2O(g)$\rarr$H2O(l) 2)2NO(g)$\rarr$N2(g)+ O2(g) 3)MgCO3(s)$\rarr$MgO(s)+ CO2(g)

A) 1 < 2 < 3 B) 2 < 3 < 1 C) 3 < 2 < 1 D) 2 < 1 < 3 E) 1 < 3 < 2 A) 1 < 2 < 3 B) 2 < 3 < 1 C) 3 < 2 < 1 D) 2 < 1 < 3 E) 1 < 3 < 2

Predict the normal boiling point of triethylborane (C6H15B)using the following data:

A) 92°C B) -21°C C) 21°C D) 365°C E) 256°C A) 92°C B) -21°C C) 21°C D) 365°C E) 256°C

Exam 17: Entropy Free Energy and Equilibrium

For the reaction CuS(s)+ H₂(g) $For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), \Delta G°f (CuS)= -53.6 kJ/mol \Delta G°f (H2S)= -33.6 kJ/mol \Delta H°f (CuS)= -53.1 kJ/mol \Delta H°f (H2S)= - 20.6 kJ/mol Calculate the value of the equilibrium constant (Kp)for this reaction at 298 K.$ H₂S(g)+ Cu(s), $\Delta$ G°_f (CuS)= -53.6 kJ/mol $\Delta$ G°_f (H₂S)= -33.6 kJ/mol $\Delta$ H°_f (CuS)= -53.1 kJ/mol $\Delta$ H°_f (H₂S)= - 20.6 kJ/mol Calculate the value of the equilibrium constant (K_p)for this reaction at 298 K.

(Short Answer)

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Question 81

Which one of the following reactions would you expect to have the lowest $\Delta$ S°?

(Multiple Choice)

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Question 82

For the reaction SbCl₅(g) $For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), \Delta G°f (SbCl5)= -334.34 kJ/mol \Delta G°f (SbCl3)= -301.25 kJ/mol \Delta H°f (SbCl5)= -394.34 kJ/mol \Delta H°f (SbCl3)= -313.80 kJ/mol Calculate the value of the equilibrium constant (Kp)for this reaction at 298 K.$ SbCl₃(g)+ Cl₂(g), $\Delta$ G°_f (SbCl₅)= -334.34 kJ/mol $\Delta$ G°_f (SbCl₃)= -301.25 kJ/mol $\Delta$ H°_f (SbCl₅)= -394.34 kJ/mol $\Delta$ H°_f (SbCl₃)= -313.80 kJ/mol Calculate the value of the equilibrium constant (K_p)for this reaction at 298 K.

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Question 83

Which of these species has the highest entropy (S°)at 25°C?

(Multiple Choice)

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Question 84

At 700 K, the equilibrium constant for the reaction CO(g)+ H₂O(g) $At 700 K, the equilibrium constant for the reaction CO(g)+ H2O(g) CO2(g)+ H2(g)is 5.10.What is \Delta G° for this reaction at this temperature?$ CO₂(g)+ H₂(g)is 5.10.What is $\Delta$ G° for this reaction at this temperature?

(Short Answer)

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Question 85

For the reaction 3H₂(g)+ N₂(g) 2NH₃(g), K_c = 9.0 at 350°C.In what direction does the reaction proceed when 1.0 mol NH₃, 5.0 mol N₂, and 5.0 mol H₂ are mixed in a 2.5 L reactor?

(Short Answer)

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Question 86

Which of the following is consistent with a reaction at equilibrium?

(Multiple Choice)

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Question 87

Calculate $\Delta$ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) $\rarr$ 2Pb(s)+ CO₂(g)given these absolute entropies: $Calculate \Delta S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) \rarr 2Pb(s)+ CO2(g)given these absolute entropies:$

(Multiple Choice)

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Question 88

Calculate the equilibrium constant for the decomposition of water 2H₂O(l) $Calculate the equilibrium constant for the decomposition of water 2H2O(l) 2H2(g)+ O2(g) At 25°C, given that \Delta G°f (H2O(l))= -237.2 kJ/mol.$ 2H₂(g)+ O₂(g) At 25°C, given that $\Delta$ G°_f(H₂O(l))= -237.2 kJ/mol.

(Multiple Choice)

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Question 89

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.Find K_p for the reaction H₂(g)+ I₂(s) 2HI(g)at this temperature.

(Multiple Choice)

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Question 90

For the reaction 2 SO₂(g)+ O₂(g) $\rarr$ 2 SO₃(g), if initially P(SO₂)= 1.2 atm, P(O₂)= 1.8 atm, and P(SO₃)= 2.1 atm, calculate $\Delta$ G for this reaction at 25°C.The following data is valid at 25°C: $For the reaction 2 SO2(g)+ O2(g) \rarr 2 SO3(g), if initially P(SO2)= 1.2 atm, P(O2)= 1.8 atm, and P(SO3)= 2.1 atm, calculate \Delta G for this reaction at 25°C.The following data is valid at 25°C:$

(Multiple Choice)

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Question 91

In the gas phase, formic acid forms a dimmer, 2HCOOH(g) $In the gas phase, formic acid forms a dimmer, 2HCOOH(g) (HCOOH)2(g).For this reaction, \Delta H° = -60.1 kJ/mol and \Delta G° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (Kp)for this reaction at 75 °C.$ (HCOOH)₂(g).For this reaction, $\Delta$ H° = -60.1 kJ/mol and $\Delta$ G° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (K_p)for this reaction at 75 °C.

(Multiple Choice)

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Question 92

Arrange these reactions according to increasing $\Delta$ S. 1)H₂O(g) $\rarr$ H₂O(l) 2)2NO(g) $\rarr$ N₂(g)+ O₂(g) 3)MgCO₃(s) $\rarr$ MgO(s)+ CO₂(g)

(Multiple Choice)

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Question 93

For the reaction SbCl₅(g) $For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), \Delta G°f (SbCl5)= -334.34 kJ/mol \Delta G°f (SbCl3)= -301.25 kJ/mol \Delta H°f (SbCl5)= -394.34 kJ/mol \Delta H°f (SbCl3)= -313.80 kJ/mol Calculate \Delta G at 800 K and 1 atm pressure (assume \Delta S° and \Delta H° do not change with temperature).$ SbCl₃(g)+ Cl₂(g), $\Delta$ G°_f (SbCl₅)= -334.34 kJ/mol $\Delta$ G°_f (SbCl₃)= -301.25 kJ/mol $\Delta$ H°_f (SbCl₅)= -394.34 kJ/mol $\Delta$ H°_f (SbCl₃)= -313.80 kJ/mol Calculate $\Delta$ G at 800 K and 1 atm pressure (assume $\Delta$ S°and $\Delta$ H° do not change with temperature).

(Short Answer)

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Question 94

Which of these species would you expect to have the lowest standard entropy (S°)?

(Multiple Choice)

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Question 95

Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO₃(s) $\rarr$ Na₂CO₃(s)+ CO₂(g)+ H₂O(g) Given that $\Delta$ H° = 128.9 kJ/mol and $\Delta$ G° = 33.1 kJ/mol at 25°C, above what minimum temperature will the reaction become spontaneous under standard state conditions?

(Multiple Choice)

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Question 96

Given the following data, calculate the boiling point of HCOOH (formic acid).

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Question 97

For the reaction H₂O₂(g) $\rarr$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C.Is H₂O₂(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

(Short Answer)

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Question 98

Predict the normal boiling point of triethylborane (C₆H₁₅B)using the following data:

(Multiple Choice)

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Question 99

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br2, assuming that \Delta S° and \Delta H° are temperature-independent.$

(Short Answer)

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Question 100

Showing 81 - 100 of 128

Which one of the following reactions would you expect to have the lowest $\Delta$ S°?

Which of these species has the highest entropy (S°)at 25°C?

For the reaction 3H₂(g)+ N₂(g) 2NH₃(g), K_c = 9.0 at 350°C.In what direction does the reaction proceed when 1.0 mol NH₃, 5.0 mol N₂, and 5.0 mol H₂ are mixed in a 2.5 L reactor?

Which of the following is consistent with a reaction at equilibrium?

Calculate $\Delta$ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) $\rarr$ 2Pb(s)+ CO₂(g)given these absolute entropies: $Calculate \Delta S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) \rarr 2Pb(s)+ CO<sub>2</sub>(g)given these absolute entropies:$

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.Find K_p for the reaction H₂(g)+ I₂(s) 2HI(g)at this temperature.

Arrange these reactions according to increasing $\Delta$ S. 1)H₂O(g) $\rarr$ H₂O(l) 2)2NO(g) $\rarr$ N₂(g)+ O₂(g) 3)MgCO₃(s) $\rarr$ MgO(s)+ CO₂(g)

Which of these species would you expect to have the lowest standard entropy (S°)?

Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO₃(s) $\rarr$ Na₂CO₃(s)+ CO₂(g)+ H₂O(g) Given that $\Delta$ H° = 128.9 kJ/mol and $\Delta$ G° = 33.1 kJ/mol at 25°C, above what minimum temperature will the reaction become spontaneous under standard state conditions?

Given the following data, calculate the boiling point of HCOOH (formic acid).

For the reaction H₂O₂(g) $\rarr$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C.Is H₂O₂(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Predict the normal boiling point of triethylborane (C₆H₁₅B)using the following data:

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br<sub>2</sub>, assuming that \Delta S° and \Delta H° are temperature-independent.$

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Exam 17: Entropy Free Energy and Equilibrium

For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), Δ\DeltaΔ G°f (CuS)= -53.6 kJ/mol Δ\DeltaΔ G°f (H2S)= -33.6 kJ/mol Δ\DeltaΔ H°f (CuS)= -53.1 kJ/mol Δ\DeltaΔ H°f (H2S)= - 20.6 kJ/mol Calculate the value of the equilibrium constant (Kp)for this reaction at 298 K.

Which one of the following reactions would you expect to have the lowest Δ\DeltaΔ S°?

For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), Δ\DeltaΔ G°f (SbCl5)= -334.34 kJ/mol Δ\DeltaΔ G°f (SbCl3)= -301.25 kJ/mol Δ\DeltaΔ H°f (SbCl5)= -394.34 kJ/mol Δ\DeltaΔ H°f (SbCl3)= -313.80 kJ/mol Calculate the value of the equilibrium constant (Kp)for this reaction at 298 K.

Which of these species has the highest entropy (S°)at 25°C?

At 700 K, the equilibrium constant for the reaction CO(g)+ H2O(g) CO2(g)+ H2(g)is 5.10.What is Δ\DeltaΔ G° for this reaction at this temperature?

For the reaction 3H2(g)+ N2(g) 2NH3(g), Kc = 9.0 at 350°C.In what direction does the reaction proceed when 1.0 mol NH3, 5.0 mol N2, and 5.0 mol H2 are mixed in a 2.5 L reactor?

Which of the following is consistent with a reaction at equilibrium?

Calculate Δ\DeltaΔ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) →\rarr→ 2Pb(s)+ CO2(g)given these absolute entropies:

Calculate the equilibrium constant for the decomposition of water 2H2O(l) 2H2(g)+ O2(g) At 25°C, given that Δ\DeltaΔ G°f (H2O(l))= -237.2 kJ/mol.

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.Find Kp for the reaction H2(g)+ I2(s) 2HI(g)at this temperature.

For the reaction 2 SO2(g)+ O2(g) →\rarr→ 2 SO3(g), if initially P(SO2)= 1.2 atm, P(O2)= 1.8 atm, and P(SO3)= 2.1 atm, calculate Δ\DeltaΔ G for this reaction at 25°C.The following data is valid at 25°C:

In the gas phase, formic acid forms a dimmer, 2HCOOH(g) (HCOOH)2(g).For this reaction, Δ\DeltaΔ H° = -60.1 kJ/mol and Δ\DeltaΔ G° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (Kp)for this reaction at 75 °C.

Arrange these reactions according to increasing Δ\DeltaΔ S. 1)H2O(g) →\rarr→ H2O(l) 2)2NO(g) →\rarr→ N2(g)+ O2(g) 3)MgCO3(s) →\rarr→ MgO(s)+ CO2(g)

Which of these species would you expect to have the lowest standard entropy (S°)?

Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s) →\rarr→ Na2CO3(s)+ CO2(g)+ H2O(g) Given that Δ\DeltaΔ H° = 128.9 kJ/mol and Δ\DeltaΔ G° = 33.1 kJ/mol at 25°C, above what minimum temperature will the reaction become spontaneous under standard state conditions?

Given the following data, calculate the boiling point of HCOOH (formic acid).

For the reaction H2O2(g) →\rarr→ H2O(g)+ 1/2O2(g), Δ\DeltaΔ H° = -106 kJ/mol and Δ\DeltaΔ S° = 58 J/K·mol at 25°C.Is H2O2(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Predict the normal boiling point of triethylborane (C6H15B)using the following data:

Given the following data, estimate the boiling point of bromine, Br2, assuming that Δ\DeltaΔ S° and Δ\DeltaΔ H° are temperature-independent.

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Which one of the following reactions would you expect to have the lowest $\Delta$ S°?

For the reaction 3H₂(g)+ N₂(g) 2NH₃(g), K_c = 9.0 at 350°C.In what direction does the reaction proceed when 1.0 mol NH₃, 5.0 mol N₂, and 5.0 mol H₂ are mixed in a 2.5 L reactor?

Calculate $\Delta$ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) $\rarr$ 2Pb(s)+ CO₂(g)given these absolute entropies: $Calculate \Delta S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) \rarr 2Pb(s)+ CO<sub>2</sub>(g)given these absolute entropies:$

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.Find K_p for the reaction H₂(g)+ I₂(s) 2HI(g)at this temperature.

Arrange these reactions according to increasing $\Delta$ S. 1)H₂O(g) $\rarr$ H₂O(l) 2)2NO(g) $\rarr$ N₂(g)+ O₂(g) 3)MgCO₃(s) $\rarr$ MgO(s)+ CO₂(g)

Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO₃(s) $\rarr$ Na₂CO₃(s)+ CO₂(g)+ H₂O(g) Given that $\Delta$ H° = 128.9 kJ/mol and $\Delta$ G° = 33.1 kJ/mol at 25°C, above what minimum temperature will the reaction become spontaneous under standard state conditions?

For the reaction H₂O₂(g) $\rarr$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C.Is H₂O₂(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?

Predict the normal boiling point of triethylborane (C₆H₁₅B)using the following data:

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br<sub>2</sub>, assuming that \Delta S° and \Delta H° are temperature-independent.$