Chapter 17, Problem 16A

Interpretation Introduction

Interpretation:

The graph that represents the reaction between nitrogen and hydrogen gas to produce ammonia have to be explained.

Concept Introduction:

Chemical equilibrium: Chemical equilibrium is a state of a chemical reaction when the rate of forward reaction is equal to the rate of backward reaction. The chemical reaction follows the law of mass action. The law of mass action states that the rate of a chemical reaction is directly proportional to the product of active masses of the reactants.

Explanation of Solution

The given chemical equation is-

  $\begin{array}{l}{N}_2(s)+3H_2(g)\rightleftharpoons 2N{H}_3(g)\\ K_{eq}=\frac{{[N{H}_3]}^2}{[N_2]{[H_2]}^3}\end{array}$

  

Initially the concentration of the product NH₃is zero. The concentration of NH₃gradually increases with time and the concentration of H₂ and N₂gradually decrease with time. The rate of decrease in the concentration of H₂ is higher than concentration of N₂as more number of H₂ molecules are consumed in the course of the reaction. After a certain time, the concentrations of reactants and products are no longer changing. That means the reaction is in equilibrium. All concentrations become constant asthe horizontal lines in the graphremain constant.