At 623K, the equilibrium constant Kc for the reactions N2+3H2=2NH3 is 2.37x10^-3. In a certain experiment, the equilibrium concentrations are 0.683, 8.8 and 1.05M for N2, H2 and NH3 respectively. Adsuming more NH3 is added to the mixture to increase it's concentration to 3.65M a)Use Le Chanteliers principle to predict the direction that the net reaction will shift to re-establish equilibrium b)confirm your prediction

Question

At 623K, the equilibrium constant Kc for the reactions N2+3H2=2NH3 is 2.37x10^-3. In a certain experiment, the equilibrium concentrations are 0.683, 8.8 and 1.05M for N2, H2 and NH3 respectively. Adsuming more NH3 is added to the mixture to increase it's concentration to 3.65M a)Use Le Chanteliers principle to predict the direction that the net reaction will shift to re-establish equilibrium b)confirm your prediction

Answer 1

a) According to Le Chatelier's principle, if the concentration of NH3 is increased, the reaction will shift in the reverse direction to decrease the concentration of NH3 and re-establish equilibrium. Therefore, the net reaction will shift to the left (from NH3 to N2 and H2).

b) To confirm our prediction, let's calculate the new equilibrium constant Kc using the new concentrations:

Kc = [NH3]^2 / ([N2][H2])

Kc = (3.65)^2 / (0.683)(8.8)

Kc = 13.3225 / 6.0104

Kc ≈ 2.22

Since the new Kc value is closer to 2.37x10^-3 than the original value, the reaction will indeed shift to the left to decrease the concentration of NH3 and re-establish equilibrium.