Chapter 13, Problem 111SAE

Interpretation Introduction

Interpretation:

The correct option from the following should be selected for a reaction when $\text{ΔrG}°\text{ = 0 }$ for the reaction:

K = 0; K =1; ${\text{Δ}}_{\text{r}}{\text{H}}^{\text{o}}\text{ = 0}$; ${\text{Δ}}_{\text{r}}{\text{S}}^{\text{o}}\text{ = 0}$; the equilibrium activities of the reactants and products do not depend on the initial conditions.

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:

$\text{ΔrG}°\text{ = ΔrH}°\text{ - TΔrS}°$

${\text{K}}_{\text{p}}$ or $\text{Kc}$ are the equilibrium constants for the reaction which are ratio of gaseous and aqueous products and reactant molecules. The relation between equilibrium constant and $\Delta \text{rG}°$ can be written as:

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