Question

State and explain Le Chatelier's principle. Apply the principle to the following equilibria.

(ii) $2{\mathrm{NH}}_3\rightleftharpoons {\mathrm{N}}_2+3{\mathrm{H}}_2-\text{Heat}$

Answer 1

1. According to Le Chatelier's principle principle, when a system at equilibrium is subjected to a constraint or change, the position of the equilibrium shifts in a direction that opposes the constraints.
2. The given reaction is: $$\begin{gathered} 2{\mathrm{NH}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)-\text{Heat} \\ \mathrm{Ammonia}\mathrm{Nitrogen}\mathrm{Hydrogen} \end{gathered}$$
3. This reaction is an endothermic reaction as heat is absorbed during this.
4. Now, applying Le-Chatelier's principle to this reaction, when the temperature is increased, that means more heat is added, this will shift the equilibrium to the right side.
5. And on decreasing the temperature, an endothermic temperature shifts towards the reactants side to counteract the loss of heat,