Chapter 14, Problem 14.1QP

Interpretation Introduction

Interpretation:

Equilibrium has to be explained briefly. Two examples of a dynamic equilibrium have to be given.

Concept introduction:

• Chemical equation is the representation of a chemical reaction, in which the reactants and products of the reactions are represented left and right side of an arrow respectively by using their respective chemical formulas.
• Chemical equilibrium is achieved when the rate of the forward reaction becomes equal to the rate of the forward reaction.
• The concept of dynamic equilibrium occurs in reversible reactions where the concentration and rate of formation of reactants and products are same.

Explanation of Solution

Equilibrium of a reaction where both reactant and products has completely different chemical compositions is termed as chemical equilibrium. In chemical equilibrium, the rate of forward and backward reaction remains same and also reactant and product concentration is constant.

Two examples of a dynamic equilibrium are given below:

Production of nitrogen dioxide $\left(N{O}_2\right)$ by the decomposition of dinitrogen tetroxide $\left({\text{N}}_{\text{2}}{\text{O}}_{\text{4}}\right)$ can be given as:

$N_2{O}_{4\left(g\right)}\underset{}{\rightleftharpoons }{\text{NO}}_{\text{2(g)}}$

Reaction between carbon monoxide $\left(\text{CO}\right)$  and chlorine gas $\left({\text{Cl}}_2\right)$  to form phosgene $\left(COC{l}_2\right)$ can be given as:

${\text{CO}}_{\text{(g)}}\text{+}C{l}_{\text{2(g)}}\underset{}{\rightleftharpoons }{\text{COCl}}_{\text{2(g)}}$

In both cases the double arrow represents that the reaction is reversible.