The equation for the reaction that occurs during ammonia manufacture is shown. $\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)$ $\Delta H = -92\,\text{kJ mol}^{-1}$ The reaction is performed at about $200$ atmospheres pressure, with an iron catalyst, and at temperatures from $350\,^{\circ}\text{C}$ to $450\,^{\circ}\text{C}$. Which statement is incorrect?
- AAt higher temperatures the amount of ammonia present at equilibrium is less.
- BChanging the pressure has no effect on the rate of reaction.
- CThe catalyst is used to speed up the reaction.
- DWhen the reaction is at equilibrium, the forward reaction is taking place at the same rate as the backward reaction.