For the reaction N2(g) + 3H2(g) ↔ 2NH3(g), the equilibrium constant, K, = 9.83 x 10-2 at a certain temperature and pressure.
While the reaction was proceeding at this temperature and pressure the concentrations of the reactants and products were measured and found to be
[N2] = 0.910 mol/L
[H2] = 0.300 mol/L
[NH3] = 0.0081 mol/L
a. Was the reaction at equilibrium? Explain. (4 marks)
b. If the reaction was not at equilibrium, in which direction was it proceeding? Explain
