Question

A gaseous catalyst X is added in a equilibrium mixture of $N_2,H_2$ and $N{H}_3$ gases at 298 K keeping pressure constant What will be observed at equilibrium reaction: $N_{2\left(g\right)}+3H_{2\left(g\right)}\rightleftharpoons 2N{H}_{3\left(g\right)}$

• A. Equitibrium will be unaffected
• B. more $N{H}_3$ gas will be formed
• C. Dissociation of Ammonia will be favoured
• D. Catalyst will change the value of equilibrium constant

Answer 1

The correct option is C Dissociation of Ammonia will be favoured

On adding the gaseous catalyst there will be no effect of catalyst on the equlibilium . But when the pressure is constant then we have to maintain the pressure then increase the volume of container than

According to the le chatelier's principal on increase the volume of the container the equilibrium will shift on the direction where the no. of mole of gas is more that why dissociation of ammonia will be favoured