Consider the following reaction equation
N\(_{2}\)(g) + 3H\(_{2(g)}\) ⇌ 2NH3(g) ∆H = -92kJ
Increasing the temperature of the reaction would
A.
shift the equilibrium to the right
B.
increase the yield of ammonia
C.
decrease the amount of hydrogen
D.
decrease the yield of ammonia
Correct answer is D
In this case, an increase in in temperature will cause the equilibrium position to shift to the left thereby decreasing the yield of ammonia.
