The Haber process, with a catalyst present, can be used to show ammonia formation as the equation below. $\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \qquad \Delta H = -92\ \text{kJ mol}^{-1}$ Which change in conditions would raise both the speed of ammonia production and the equilibrium amount of ammonia?
- Adecrease in the temperature
- Bincrease in the temperature
- Cincrease in the pressure
- Dincrease in the surface area of the catalyst