For the reaction: CO(g)+ 2 H2(g)→ CH3OH(g) Kp = 91.4 at 350 K and Kp = 2.05 × 10-4 at 298 K. What is the value of ΔrH°?

A) 49.9 kJ/mol B) 2.08 × 103 kJ/mol C) 3.74 × 10-2 kJ/mol D) 217 kJ/mol E) 446 kJ/mol A) 49.9 kJ/mol B) 2.08 × 103 kJ/mol C) 3.74 × 10-2 kJ/mol D) 217 kJ/mol E) 446 kJ/mol

The equilibrium constant for the reaction below is 7.2 × 10-4 at 298 K and 1 atm. HNO2(aq)+ H2O(l)⇌ NO2-(aq)+ H3O+(aq) Which of the below statements is TRUE under the following conditions: [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0 × 10-5 M

A) the reaction is at equilibrium B) the forward reaction is spontaneous C) the reverse reaction is spontaneous D) the forward reaction is endothermic E) the reverse reaction is exothermic A) the reaction is at equilibrium B) the forward reaction is spontaneous C) the reverse reaction is spontaneous D) the forward reaction is endothermic E) the reverse reaction is exothermic

Calculate the temperature for which Keq for a reaction is 1.04 × 103 where ΔrH° = -83.2 kJ/mol and ΔrS° = -246 J/mol K.

A) 0.274 K B) 307 K C) 0.307 K D) 274 K E) cannot be determined without ΔrG° A) 0.274 K B) 307 K C) 0.307 K D) 274 K E) cannot be determined without ΔrG°

Exam 13: Spontaneous Change: Entropy and Gibbs Energy

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Ethanol ( OH)melts at -114 °C.The enthalpy of fusion is 5.02 kJ mol^-1.The specific heats of solid and liquid ethanol are 0.97 J g^-1 °C^-1 and 2.3 J g^-1 °C^-1,respectively.How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C?

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Question 1

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What is Δ_rH° for a reaction that has K_p = 1.456 at 273 K and K_p = 14.2 at 298 K?

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Question 2

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For CO(g)+ H₂(g)→ H₂CO(g),Δ_rH° = -5.36 kJ/mol,and Δ_rS° = -109.8 J/mol K.What is the temperature at which K_eq is 1.0 × 10^-2?

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Question 3

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For the reaction: CO(g)+ 2 H₂(g)→ CH₃OH(g) K_p = 91.4 at 350 K and K_p = 2.05 × 10^-4 at 298 K. What is the value of Δ_rH°?

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Question 4

How much heat is released when 85.0 g of steam at 100.0 °C is cooled to ice at -15.0 °C? The enthalpy of vaporization of water is 40.67 kJ mol^-1,the enthalpy of fusion for water is 6.01 kJ mol^-1,the molar heat capacity of liquid water is 75.4 J mol^-1 °C^-1,and the molar heat capacity of ice is 36.4 J mol^-1 °C^-1.

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Question 5

Which of the following substances under equal conditions and in the same phase has the greatest molar entropy?

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Question 6

Which of the listed reactions would couple with the following reaction to produce silver? Ag₂O(s)→ 2 Ag(s)+ 1/2 O(g)Δ_rG° = 11.2 kJ/mol

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Question 7

The equilibrium constant for the reaction below is 7.2 × 10^-4 at 298 K and 1 atm. HNO₂(aq)+ H₂O(l)⇌ NO₂^-(aq)+ H₃O⁺(aq) Which of the below statements is TRUE under the following conditions: [HNO₂(aq)] = 1.0 M and [NO₂^-(aq)] = [H₃O⁺(aq)] = 1.0 × 10^-5M

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Question 8

The normal melting and boiling points of SO₂ are 198 and 263 K,respectively.For a plot of the standard molar entropy of SO₂ versus temperature,which of the following is INCORRECT?

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Question 9

The Gibbs energy change for a reaction is -298 kJ.The reaction is therefore:

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Question 10

For the reaction PCl₅ (g)⇌ PCl₃ (g)+ Cl₂ (g),K_c = 0.0454 at 261 °C.If a vessel is filled with theses gases such that the initial concentrations are [PCl₅] = 0.2 M,[PCl₃] = 0.2 M,and [Cl₂] = 2.25 M,which of the following statements is TRUE?

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Question 11

Choose the INCORRECT statement about coupled reactions.

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Question 12

Consider the following reaction: What is Δ_rG° for this reaction in kJ?

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Question 13

Standard Gibbs energy of formation requires the reactants be compounds in their standard state.

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Question 14

Consider the reaction: AB(g)→ A(g)+ B(g) (K_eq = 0.729 at 20 °C Δ_rH° = 45.9 kJ/mol) What is K_eq for this reaction at 377 K?

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Question 15

Which of the following combinations of signs for △H and △S will always result in a reaction being non spontaneous?

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Question 16

Which of the following processes would result in a decrease in system entropy?

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Question 17

Consider the following reaction: What is Δ_rS° for this reaction in J/mol K?

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Question 18

As the activity a of a substances increases so does its chemical potential m.

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Question 19

Calculate the temperature for which K_eq for a reaction is 1.04 × 10³ where Δ_rH° = -83.2 kJ/mol and Δ_rS° = -246 J/mol K.

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Question 20

Showing 1 - 20 of 123

Exam 13: Spontaneous Change: Entropy and Gibbs Energy

Ethanol ( OH)melts at -114 °C.The enthalpy of fusion is 5.02 kJ mol-1.The specific heats of solid and liquid ethanol are 0.97 J g-1 °C-1 and 2.3 J g-1 °C-1,respectively.How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C?

What is ΔrH° for a reaction that has Kp = 1.456 at 273 K and Kp = 14.2 at 298 K?

For CO(g)+ H2(g)→ H2CO(g),ΔrH° = -5.36 kJ/mol,and ΔrS° = -109.8 J/mol K.What is the temperature at which Keq is 1.0 × 10-2?

For the reaction: CO(g)+ 2 H2(g)→ CH3OH(g) Kp = 91.4 at 350 K and Kp = 2.05 × 10-4 at 298 K. What is the value of ΔrH°?

Which of the following substances under equal conditions and in the same phase has the greatest molar entropy?

Which of the listed reactions would couple with the following reaction to produce silver? Ag2O(s)→ 2 Ag(s)+ 1/2 O(g)ΔrG° = 11.2 kJ/mol

The equilibrium constant for the reaction below is 7.2 × 10-4 at 298 K and 1 atm. HNO2(aq)+ H2O(l)⇌ NO2-(aq)+ H3O+(aq) Which of the below statements is TRUE under the following conditions: [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0 × 10-5 M

The normal melting and boiling points of SO2 are 198 and 263 K,respectively.For a plot of the standard molar entropy of SO2 versus temperature,which of the following is INCORRECT?

The Gibbs energy change for a reaction is -298 kJ.The reaction is therefore:

For the reaction PCl5 (g)⇌ PCl3 (g)+ Cl2 (g),Kc = 0.0454 at 261 °C.If a vessel is filled with theses gases such that the initial concentrations are [PCl5] = 0.2 M,[PCl3] = 0.2 M,and [Cl2] = 2.25 M,which of the following statements is TRUE?

Choose the INCORRECT statement about coupled reactions.

Consider the following reaction: What is ΔrG° for this reaction in kJ?

Standard Gibbs energy of formation requires the reactants be compounds in their standard state.

Consider the reaction: AB(g)→ A(g)+ B(g) (Keq = 0.729 at 20 °C ΔrH° = 45.9 kJ/mol) What is Keq for this reaction at 377 K?

Which of the following combinations of signs for △H and △S will always result in a reaction being non spontaneous?

Which of the following processes would result in a decrease in system entropy?

Consider the following reaction: What is ΔrS° for this reaction in J/mol K?

As the activity a of a substances increases so does its chemical potential m.

Calculate the temperature for which Keq for a reaction is 1.04 × 103 where ΔrH° = -83.2 kJ/mol and ΔrS° = -246 J/mol K.

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Ethanol ( OH)melts at -114 °C.The enthalpy of fusion is 5.02 kJ mol^-1.The specific heats of solid and liquid ethanol are 0.97 J g^-1 °C^-1 and 2.3 J g^-1 °C^-1,respectively.How much heat (kJ)is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C?

What is Δ_rH° for a reaction that has K_p = 1.456 at 273 K and K_p = 14.2 at 298 K?

For CO(g)+ H₂(g)→ H₂CO(g),Δ_rH° = -5.36 kJ/mol,and Δ_rS° = -109.8 J/mol K.What is the temperature at which K_eq is 1.0 × 10^-2?

For the reaction: CO(g)+ 2 H₂(g)→ CH₃OH(g) K_p = 91.4 at 350 K and K_p = 2.05 × 10^-4 at 298 K. What is the value of Δ_rH°?

Which of the listed reactions would couple with the following reaction to produce silver? Ag₂O(s)→ 2 Ag(s)+ 1/2 O(g)Δ_rG° = 11.2 kJ/mol

The equilibrium constant for the reaction below is 7.2 × 10^-4 at 298 K and 1 atm. HNO₂(aq)+ H₂O(l)⇌ NO₂^-(aq)+ H₃O⁺(aq) Which of the below statements is TRUE under the following conditions: [HNO₂(aq)] = 1.0 M and [NO₂^-(aq)] = [H₃O⁺(aq)] = 1.0 × 10^-5M

The normal melting and boiling points of SO₂ are 198 and 263 K,respectively.For a plot of the standard molar entropy of SO₂ versus temperature,which of the following is INCORRECT?

For the reaction PCl₅ (g)⇌ PCl₃ (g)+ Cl₂ (g),K_c = 0.0454 at 261 °C.If a vessel is filled with theses gases such that the initial concentrations are [PCl₅] = 0.2 M,[PCl₃] = 0.2 M,and [Cl₂] = 2.25 M,which of the following statements is TRUE?

Consider the following reaction: What is Δ_rG° for this reaction in kJ?

Consider the reaction: AB(g)→ A(g)+ B(g) (K_eq = 0.729 at 20 °C Δ_rH° = 45.9 kJ/mol) What is K_eq for this reaction at 377 K?

Consider the following reaction: What is Δ_rS° for this reaction in J/mol K?

Calculate the temperature for which K_eq for a reaction is 1.04 × 10³ where Δ_rH° = -83.2 kJ/mol and Δ_rS° = -246 J/mol K.