The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [ G = H − T S ] . Concept introduction: In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition. Given: For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19 For CO 2 , ?H = - 393.5052 kJ/ mol and ?S = 213.676 For CaCO 3 , ?H = - 1206.91 kJ/ mol and ?S = 88.701 We need to calculate the value of k p at 25 °C for the given reaction.

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Answer 1

Question

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

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Answer 2

Question

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

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Answer 3

Question

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

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Answer 4

Question

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

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Answer 5

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

Answer 6

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

Answer 7

Chapter 17, Problem 17.19P

Interpretation Introduction

Interpretation:

The given problem can solved by the relation between gibbs free energy, enthalpy, and entropy [G = H−TS].

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. The free energy is the minimum thermodynamic potential at which the system remains at chemical equilibrium under constant temperature and pressure condition.

Given:

For CaO, ?H = - 635.12 kJ/ mol and ?S = 38.19

For CO₂, ?H = - 393.5052 kJ/ mol and ?S = 213.676

For CaCO₃, ?H = - 1206.91 kJ/ mol and ?S = 88.701

We need to calculate the value of k_p at 25 °C for the given reaction.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 17 - Prob. 17.1P Ch. 17 - Prob. 17.2P Ch. 17 - Prob. 17.3A Ch. 17 - Prob. 17.4P Ch. 17 - Prob. 17.5P Ch. 17 - Prob. 17.6A Ch. 17 - Prob. 17.7P Ch. 17 - Prob. 17.8A Ch. 17 - Prob. 17.9P Ch. 17 - APPLY 17.10 Use the values of Hf and S in Appendix...

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