Question

For the reaction $2N{H}_3\left(g\right)\rightleftharpoons N_2\left(g\right)+3H_2\left(g\right),\Delta H=93.6kJmo{l}^{-1}$. Which of the following facts does not hold well?

• A. The pressure changes at constant temperature do not affect the equilibrium constant
• B. The volume changes at constant temperature do not affect the equilibrium constant
• C. The dissociation of is more favored at high temperature
• D. The dissociation of is less favored at high temperature

Answer 1

The correct option is D

The dissociation of is less favored at high temperature

We can write the given reaction as $2N{H}_3\left(g\right)+Q\rightleftharpoons N_2\left(g\right)+3H_2\left(g\right)$. Increasing temperature implies heat is added. This will shift the equilibrium to right side, i.e. more of $N{H}_3$ is dissociated.