Calculate $\Delta$G° for the reaction 3NO2(g)+ H2O(l)$\to$ 2HNO3(l)+ NO(g).

A) 8.7 kJ/mol B) 192 kJ/mol C) -414 kJ/mol D) -192 kJ/mol E) -155 kJ/mol A) 8.7 kJ/mol B) 192 kJ/mol C) -414 kJ/mol D) -192 kJ/mol E) -155 kJ/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 $\times$ 10-84 C) 2.5 $\times$ 10-42 D) 1.6 $\times$ 1083 E) 4.7 $\times$ 105 A) 0.83 B) 6.3 $\times$ 10-84 C) 2.5 $\times$ 10-42 D) 1.6 $\times$ 1083 E) 4.7 $\times$ 105

At 1500°C the equilibrium constant for the reaction CO(g)+ 2H2(g) CH3OH(g)has the value Kp = 1.4 $\times$10-7. Calculate $\Delta$G° for this reaction at 1500°C.

A) 105 kJ/mol B) 1.07 kJ/mol C) -233 kJ/mol D) -105 kJ/mol E) 233 kJ/mol A) 105 kJ/mol B) 1.07 kJ/mol C) -233 kJ/mol D) -105 kJ/mol E) 233 kJ/mol

For the reaction H2(g)+ S(s)$ \to$ H2S(g), $\Delta$H° = -20.2 kJ/mol and $\Delta$S° = +43.1 J/K·mol.Which of these statements is true?

A) The reaction is only spontaneous at low temperatures. B) The reaction is spontaneous at all temperatures. C) ($\Delta$G° becomes less favorable as temperature increases.) D) The reaction is spontaneous only at high temperatures. E) The reaction is at equilibrium at 25°C under standard conditions. A) The reaction is only spontaneous at low temperatures. B) The reaction is spontaneous at all temperatures. C) ($\Delta$G° becomes less favorable as temperature increases.) D) The reaction is spontaneous only at high temperatures. E) The reaction is at equilibrium at 25°C under standard conditions.

For the reaction 2C(graphite)+ H2(g)$\to$ C2H2(g), $\Delta$G°= +209.2 kJ/mol at 25°C. If P(H2)= 100.atm, and P(C2H2)= 0.10 atm, calculate $\Delta$G for this reaction.

A) +207.8 kJ/mol B) +226.3 kJ/mol C) +192.1 kJ/mol D) +17.3 kJ/mol E) -16.9 kJ/mol A) +207.8 kJ/mol B) +226.3 kJ/mol C) +192.1 kJ/mol D) +17.3 kJ/mol E) -16.9 kJ/mol

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).

The answer of For the reaction SbCl5(g) SbCl3(g)+...

Which response includes all the following processes that are accompanied by an increase in entropy? 1)2SO2(g)+ O2(g)$\to$ SO3(g) 2)H2O(l)$\to$ H2O(s) 3)Br2(l)$\to$ Br2(g) 4)H2O2(l)$\to$ H2O(l)+ 1/2O2(g)

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

Exam 18: Entropy, Free Energy, and Equilibrium

Calculate $\Delta$ G° for the reaction 3NO₂(g)+ H₂O(l) $\to$ 2HNO₃(l)+ NO(g). $Calculate \Delta G° for the reaction 3NO2(g)+ H2O(l) \to 2HNO3(l)+ NO(g).$

(Multiple Choice)

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Question 81

Which species will have the greatest absolute entropy at 25°C?

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Question 82

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.

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Question 83

How does the entropy change when a liquid is vaporized?

(Short Answer)

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Question 84

The following reaction is spontaneous under standard state conditions at 25°C: AgCl(s) $\to$ Ag⁺(aq)+ Cl^-(aq)( $\Delta$ G° = 55 kJ/mol)

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Question 85

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

(Multiple Choice)

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Question 86

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

(Multiple Choice)

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Question 87

Consider the reaction CO(g)+ 2H₂(g) $Consider the reaction CO(g)+ 2H2(g) CH3OH(l)at 25°C. \Delta G°f (CO)= -137.3 kJ/mol \Delta G°f (CH3OH)= -166.3 kJ/mol \Delta H°f (CO)= -110.5 kJ/mol \Delta H°f (CH3OH)= -238.7 kJ/mol S°(CO)= 197.9 J/K·mol S°(CH3OH)= 126.8 J/K·mol Calculate value of the equilibrium constant (Kp)for this reaction at 25°C.$ CH₃OH(l)at 25°C. $\Delta$ G°_f (CO)= -137.3 kJ/mol $\Delta$ G°_f (CH₃OH)= -166.3 kJ/mol $\Delta$ H°_f (CO)= -110.5 kJ/mol $\Delta$ H°_f (CH₃OH)= -238.7 kJ/mol S°(CO)= 197.9 J/K·mol S°(CH₃OH)= 126.8 J/K·mol Calculate value of the equilibrium constant (K_p)for this reaction at 25°C.

(Short Answer)

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Question 88

At 1500°C the equilibrium constant for the reaction CO(g)+ 2H₂(g) $At 1500°C the equilibrium constant for the reaction CO(g)+ 2H2(g) CH3OH(g)has the value Kp = 1.4 \times 10-7. Calculate \Delta G° for this reaction at 1500°C.$ CH₃OH(g)has the value K_p = 1.4 $\times$ 10^-7. Calculate $\Delta$ G° for this reaction at 1500°C.

(Multiple Choice)

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Question 89

For the reaction H₂(g)+ S(s) $\to$ H₂S(g), $\Delta$ H° = -20.2 kJ/mol and $\Delta$ S° = +43.1 J/K·mol.Which of these statements is true?

(Multiple Choice)

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Question 90

Assuming $\Delta$ S° and $\Delta$ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g) $\to$ H₂(g)+ CO(s)( $\Delta$ S° = 133.6 J/K·mol; $\Delta$ H° = 131.3 kJ/mol)

(Short Answer)

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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

For the reaction 2C(graphite)+ H₂(g) $\to$ C₂H₂(g), $\Delta$ G°= +209.2 kJ/mol at 25°C. If P(H₂)= 100.atm, and P(C₂H₂)= 0.10 atm, calculate $\Delta$ G for this reaction.

(Multiple Choice)

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Question 93

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 94

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 95

Using the thermodynamic data provided below, calculate K_sp for ZnS(s)at 25°.

(Essay)

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Question 96

Which response includes all the following processes that are accompanied by an increase in entropy? 1)2SO₂(g)+ O₂(g) $\to$ SO₃(g) 2)H₂O(l) $\to$ H₂O(s) 3)Br₂(l) $\to$ Br₂(g) 4)H₂O₂(l) $\to$ H₂O(l)+ ¹/₂O₂(g)

(Multiple Choice)

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Question 97

Choose the substance with the higher entropy per mole at a given temperature: Br₂(l)or Br₂(g).

(Short Answer)

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Question 98

Sulfur can be separated from lead in the mineral galena, PbS(s), by "roasting" the ore in the presence of oxygen as shown in the following reaction: 2PbS(s)+ 3O₂(g) $\to$ 2PbO(s)+ 2SO₂(g) Determine $\Delta$ G for the above reaction at 850°C. $Sulfur can be separated from lead in the mineral galena, PbS(s), by roasting the ore in the presence of oxygen as shown in the following reaction: 2PbS(s)+ 3O2(g) \to 2PbO(s)+ 2SO2(g) Determine \Delta G for the above reaction at 850°C.$

(Short Answer)

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Question 99

Choose the substance with the higher entropy per mole at a given temperature: CO₂(g)or CO₂(aq).

(Short Answer)

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Question 100

Showing 81 - 100 of 112

Calculate $\Delta$ G° for the reaction 3NO₂(g)+ H₂O(l) $\to$ 2HNO₃(l)+ NO(g). $Calculate \Delta G° for the reaction 3NO<sub>2</sub>(g)+ H<sub>2</sub>O(l) \to 2HNO<sub>3</sub>(l)+ NO(g).$

Which species will have the greatest absolute entropy at 25°C?

How does the entropy change when a liquid is vaporized?

The following reaction is spontaneous under standard state conditions at 25°C: AgCl(s) $\to$ Ag⁺(aq)+ Cl^-(aq)( $\Delta$ G° = 55 kJ/mol)

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 H₂(g)+ S(s) $\to$ H₂S(g), $\Delta$ H° = -20.2 kJ/mol and $\Delta$ S° = +43.1 J/K·mol.Which of these statements is true?

Assuming $\Delta$ S° and $\Delta$ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g) $\to$ H₂(g)+ CO(s)( $\Delta$ S° = 133.6 J/K·mol; $\Delta$ H° = 131.3 kJ/mol)

For the reaction 2C(graphite)+ H₂(g) $\to$ C₂H₂(g), $\Delta$ G°= +209.2 kJ/mol at 25°C. If P(H₂)= 100.atm, and P(C₂H₂)= 0.10 atm, calculate $\Delta$ G for this reaction.

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.

Using the thermodynamic data provided below, calculate K_sp for ZnS(s)at 25°.

Which response includes all the following processes that are accompanied by an increase in entropy? 1)2SO₂(g)+ O₂(g) $\to$ SO₃(g) 2)H₂O(l) $\to$ H₂O(s) 3)Br₂(l) $\to$ Br₂(g) 4)H₂O₂(l) $\to$ H₂O(l)+ ¹/₂O₂(g)

Choose the substance with the higher entropy per mole at a given temperature: Br₂(l)or Br₂(g).

Choose the substance with the higher entropy per mole at a given temperature: CO₂(g)or CO₂(aq).

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Exam 18: Entropy, Free Energy, and Equilibrium

Calculate Δ\DeltaΔ G° for the reaction 3NO2(g)+ H2O(l) →\to→ 2HNO3(l)+ NO(g).

Which species will have the greatest absolute entropy at 25°C?

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.

How does the entropy change when a liquid is vaporized?

The following reaction is spontaneous under standard state conditions at 25°C: AgCl(s) →\to→ Ag+(aq)+ Cl-(aq)( Δ\DeltaΔ G° = 55 kJ/mol)

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

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

At 1500°C the equilibrium constant for the reaction CO(g)+ 2H2(g) CH3OH(g)has the value Kp = 1.4 ×\times× 10-7. Calculate Δ\DeltaΔ G° for this reaction at 1500°C.

For the reaction H2(g)+ S(s) →\to→ H2S(g), Δ\DeltaΔ H° = -20.2 kJ/mol and Δ\DeltaΔ S° = +43.1 J/K·mol.Which of these statements is true?

Assuming Δ\DeltaΔ S° and Δ\DeltaΔ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H2O(g) →\to→ H2(g)+ CO(s)( Δ\DeltaΔ S° = 133.6 J/K·mol; Δ\DeltaΔ H° = 131.3 kJ/mol)

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.

For the reaction 2C(graphite)+ H2(g) →\to→ C2H2(g), Δ\DeltaΔ G°= +209.2 kJ/mol at 25°C. If P(H2)= 100.atm, and P(C2H2)= 0.10 atm, calculate Δ\DeltaΔ G for this reaction.

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.

Using the thermodynamic data provided below, calculate Ksp for ZnS(s)at 25°.

Which response includes all the following processes that are accompanied by an increase in entropy? 1)2SO2(g)+ O2(g) →\to→ SO3(g) 2)H2O(l) →\to→ H2O(s) 3)Br2(l) →\to→ Br2(g) 4)H2O2(l) →\to→ H2O(l)+ 1/2O2(g)

Choose the substance with the higher entropy per mole at a given temperature: Br2(l)or Br2(g).

Sulfur can be separated from lead in the mineral galena, PbS(s), by "roasting" the ore in the presence of oxygen as shown in the following reaction: 2PbS(s)+ 3O2(g) →\to→ 2PbO(s)+ 2SO2(g) Determine Δ\DeltaΔ G for the above reaction at 850°C.

Choose the substance with the higher entropy per mole at a given temperature: CO2(g)or CO2(aq).

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Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

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Thermo-Chemistry

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Chemical Bonding I: Basic Concepts

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Acids and Bases

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Calculate $\Delta$ G° for the reaction 3NO₂(g)+ H₂O(l) $\to$ 2HNO₃(l)+ NO(g). $Calculate \Delta G° for the reaction 3NO<sub>2</sub>(g)+ H<sub>2</sub>O(l) \to 2HNO<sub>3</sub>(l)+ NO(g).$

The following reaction is spontaneous under standard state conditions at 25°C: AgCl(s) $\to$ Ag⁺(aq)+ Cl^-(aq)( $\Delta$ G° = 55 kJ/mol)

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

For the reaction H₂(g)+ S(s) $\to$ H₂S(g), $\Delta$ H° = -20.2 kJ/mol and $\Delta$ S° = +43.1 J/K·mol.Which of these statements is true?

Assuming $\Delta$ S° and $\Delta$ H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous? C(s)+ H₂O(g) $\to$ H₂(g)+ CO(s)( $\Delta$ S° = 133.6 J/K·mol; $\Delta$ H° = 131.3 kJ/mol)

For the reaction 2C(graphite)+ H₂(g) $\to$ C₂H₂(g), $\Delta$ G°= +209.2 kJ/mol at 25°C. If P(H₂)= 100.atm, and P(C₂H₂)= 0.10 atm, calculate $\Delta$ G for this reaction.

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.

Using the thermodynamic data provided below, calculate K_sp for ZnS(s)at 25°.

Which response includes all the following processes that are accompanied by an increase in entropy? 1)2SO₂(g)+ O₂(g) $\to$ SO₃(g) 2)H₂O(l) $\to$ H₂O(s) 3)Br₂(l) $\to$ Br₂(g) 4)H₂O₂(l) $\to$ H₂O(l)+ ¹/₂O₂(g)

Choose the substance with the higher entropy per mole at a given temperature: Br₂(l)or Br₂(g).

Choose the substance with the higher entropy per mole at a given temperature: CO₂(g)or CO₂(aq).