Chapter 13, Problem 87IAE

Interpretation Introduction

Interpretation:

The temperature that converted to $\text{NO(g)}$ 1.0% from equimolar mixture of ${\text{N}}_{\text{2}}\text{(g)}$ and ${\text{O}}_{\text{2}}\text{(g)}$ according to the reaction ${\text{N}}_{\text{2}}{\text{(g) + O}}_{\text{2}}\text{(g)}\rightleftharpoons \text{2NO(g)}$ should be determined.

Concept introduction:

The Gibbs energy, G, for a system is defined by the equation,

$G=H-TS$

The Gibbs energy change, ${\Delta }_{r}G$ for a process at constant T is

${\Delta }_{r}G={\Delta }_{r}H-\text{T}{\Delta }_{r}S$

Relationship of to the Equilibrium Constant K represents by following equation,

${\Delta }_{r}G=-\text{R}T\ln \text{K}$

For the following reaction,

$\text{aA+bB}\underset{}{\rightleftharpoons }\text{cC}+\text{dD}$

The equilibrium constant, K_cfor the above equation can write as follows.

${\text{K}}_{\text{c}}\text{=}\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$

A, B, C and D should be in a gaseous or aqueous state in order to use in K_cexpression.