Chapter 15, Problem 15.101SP

Interpretation Introduction

Interpretation:

The equilibrium concentrations of ${\text{H}}_{\text{2}}{\text{, I}}_{\text{2}}$ and $\text{HI}$ at $\text{500K}$ should be calculated.

Concept introduction:

At the equilibrium condition, a constantwhich is used to express the relationship between reactants and products at the given temperature in a reversible chemical reaction, is known as equilibrium constant.

For a reversible chemical reaction:

$\text{aA + bB }\to \text{cC + dD}$

The equilibrium constant $\text{K}$ is given by the following expression:

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

Where,

Equilibrium concentration of $\text{A}$ : $\left[\text{A}\right]$

Equilibrium concentration of $\text{B}$ : $\left[\text{B}\right]$

Equilibrium concentration of $\text{C}$ : $\left[\text{C}\right]$

Equilibrium concentration of $\text{D}$ : $\left[\text{D}\right]$