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 $\text{ΔS}$, $\text{ΔH}$ and $\text{ΔG}$ with Temperature. The mathematical expression of Gibb’s equation can be written as:

$\text{ΔG = ΔH - TΔS }$

With the help of this equation we can predict the change in $\text{ΔS}$, $\text{ΔH}$ and $\text{ΔG}$. ${\text{K}}_{\text{p}}$ or $\text{Kc}$ are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

$\text{A + B }\leftrightarrow \text{C + D }$

$\text{K = Kp = }\frac{\text{[PC] [PD]}}{\text{[PA] [PB]}}$

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and $\Delta \text{rG}°$ can be written as:

$\text{ΔrG° = - 2}\text{.303 RT log K}$

Here:

• R = 8.314 J / mol .K
• T = temperature in Kelvin

Interpretation Introduction

(b)

Interpretation:

Calculate theGibbs free energy change $\text{ΔrG°}$ 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 $\text{ΔS}$, $\text{ΔH}$ and $\text{ΔG}$ with Temperature. The mathematical expression of Gibb’s equation can be written as:

$\text{ΔG = ΔH - TΔS }$

With the help of this equation we can predict the change in $\text{ΔS}$, $\text{ΔH}$ and $\text{ΔG}$. ${\text{K}}_{\text{p}}$ or $\text{Kc}$ are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

$\text{A + B }\leftrightarrow \text{C + D }$

$\text{K = Kp = }\frac{\text{[PC] [PD]}}{\text{[PA] [PB]}}$

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and $\Delta \text{rG}°$ can be written as:

$\text{ΔrG° = - 2}\text{.303 RT log K}$

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 $\text{ΔS}$, $\text{ΔH}$ and $\text{ΔG}$ with Temperature. The mathematical expression of Gibb’s equation can be written as:

$\text{ΔG = ΔH - TΔS }$

With the help of this equation we can predict the change in $\text{ΔS}$, $\text{ΔH}$ and $\text{ΔG}$. ${\text{K}}_{\text{p}}$ or $\text{Kc}$ are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules.

$\text{A + B }\leftrightarrow \text{C + D }$

$\text{K = Kp = }\frac{\text{[PC] [PD]}}{\text{[PA] [PB]}}$

Here ‘a’ represent the active mass and ‘P’ represents the partial pressure. The relation between equilibrium constant and $\Delta \text{rG}°$ can be written as:

$\text{ΔrG° = - 2}\text{.303 RT log K}$

Here:

• R = 8.314 J / mol .K
• T = temperature in Kelvin