The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 10-2 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4M.
N2 + 3H2 --> 2NH3.
a) If the concentration of the reactant H2 was increased from 1.0 x 10-2 M to 2.5 x 10-1 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift.
b) If the concentration of the reactant H2 was decreased from 1.0 x 10-2 M to 2.7 x 10-4 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift.
c) If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the equilibrium position would shift.