Chapter 6, Problem 6.30NP

Interpretation Introduction

Interpretation : The degree of dissociation of N₂O₄ in the reaction ${\text{N}}_2{\text{O}}_4\text{(g) }\rightleftharpoons {\text{ 2 NO}}_2\text{(g)}$ at $300\text{ K}$ and a total pressure of $1.50\text{ bar}$ should be calculated.

Concept Introduction :

Clausius-Clapeyron equation is represented as follows:

  $\ln \frac{K_{P_2}}{K_{P_1}}=-\frac{\Delta H}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)$

Here,

  $\begin{array}{l}{K}_P\text{ - equilibrium constant}\\ \Delta H\text{ - enthalpy change}\\ \text{R - universal gas constant}\\ \text{T - temperature}\end{array}$

Also, Gibbs free energy change is represented as follows:

  $\Delta G_R^0=-RT\ln K_P$

Here,

  $\begin{array}{l}\Delta G_R^0\text{ - Gibbs free energy change}\\ \text{R - universal gas constant}\\ \text{T - temperature}\\ {\text{K}}_p\text{ - equilibrium constant}\end{array}$