The haber process is typically carried out at a temperature of approximately 500∘c. what would happen to the rate of the forward reaction if the temperature were lowered to 100∘c?

The reaction rate would decrease

Explanation:

The equation for the Haber process is given by;

N₂(g) + 3H₂(g) ⇆ 2NH₃(g)

The reaction occurs at a temperature of 500°C Therefore, the forward reaction requires a temperature of 500°C. According to Le Chatelier's principle, if a factor affecting equilibrium is altered, the equilibrium will shift in the direction that counteracts the effect causing it. In this case, decreasing the temperature to 100°C will lower the rate of the forward reaction. Consequently, less ammonia gas will be produced as the reverse reaction is favored.