(a) Interpretation: Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction. Concept introduction: The Gibb’s equation of thermodynamic purposed a relation between ΔS , ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as: ΔG = ΔH - TΔS With the help of this equation we can predict the change in ΔS , ΔH and ΔG . K p or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules. A + B ↔ C + D K = Kp = [PC] [PD] [PA] [PB] Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and Δ rG ° can be written as: ΔrG° = - 2 .303 RT log K Here: R = 8.314 J / mol .K T = temperature in Kelvin

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Answer 1

Question

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

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Answer 2

Question

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

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Answer 3

Question

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 6

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 7

Chapter 13, Problem 53E

Interpretation Introduction

(a)

Interpretation:

Calculate the equilibrium constant at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 8

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 9

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change ΔrG° at 1000 K with the help of given moles of reactant and products for the equilibrium reaction.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 10

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 11

Interpretation Introduction

(c)

Interpretation:

Interpret the direction of reaction for the given moles of reactant and product at 1000 K.

Concept introduction:

The Gibb’s equation of thermodynamic purposed a relation between ΔS, ΔH and ΔG with Temperature. The mathematical expression of Gibb’s equation can be written as:

ΔG = ΔH - TΔS

With the help of this equation we can predict the change in ΔS, ΔH and ΔG. Kp or Kc are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

A + B ↔C + D

K = Kp = [PC] [PD][PA] [PB]

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and ΔrG° can be written as:

ΔrG° = - 2.303 RT log K

Here:

R = 8.314 J / mol .K

T = temperature in Kelvin

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

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Answer 15

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Solution Summary: The author explains the Gibb's equation of thermodynamic purposed a relation between S,

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