Chapter 20, Problem 36GQ

Interpretation Introduction

Interpretation: The equilibrium constant for the reaction $\frac{\text{1}}{\text{2}}{\text{NO}}_{\text{2}}\text{(g)}\text{+}\frac{\text{1}}{\text{2}}{\text{O}}_{\text{2}}\text{(g)}\to \text{NO}\text{(g)}$ at $\text{298}\text{K}\text{and}\text{1000}\text{K}$ should be determined.

Concept introduction:

Equilibrium constant in terms of concentration${\text{[K}}_{\text{C}}\text{]}$: Equilibrium constant can be expressed in terms of concentration.

$\begin{array}{l}\text{aA}{}_{\text{(g)}}\text{+}{\text{bB}}_{\text{(g)}}\rightleftarrows \text{cC}{}_{\text{(g)}}\text{+}\text{dD}{}_{\text{(g)}}\\ {\text{K}}_{\text{c}}\text{=}\frac{{\left[\text{C}\right]}^{\text{c}}\text{×}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}\text{×}{\left[\text{B}\right]}^{\text{b}}}\end{array}$

Equilibrium constant and Gibbs free energy:

${\text{ΔG}}^{\text{0}}=-\text{RTln}\text{K}$

Relation between Gibbs free energy , Enthalpy and Entropy:

$\begin{array}{l}\text{ΔG}\text{=}\text{ΔH-TΔS}\\ \text{ΔG-}\text{Gibbs}\text{free}\text{energy}\\ \text{ΔH-}\text{Enthalpy}\\ \text{ΔS-Entropy}\end{array}$