ICE Table Practice Questions
1. In a 7L vessel, 0.54 mol of N2 , 0.68 mol of H2 and 0.27 mol of NH3 were mixed and allowed to
come to equilibrium. It was found that at equilibrium there was 0.42 mol of H2 . Calculate the
value of the equilibrium constant for this reaction:
N2(g) + 3H2(g) ∏ 2NH3(g)
2. A 2.00 mol sample of nitrosyl bromide, NOBr was introduced into a 5.0 L vessel. At equilibrium
the concentration of nitrosyl bromide was found to be 0.0750 M. Calculate the equilibrium
constant for the reaction shown in the equation
2NOBr (g) ∏ 2NO (g) + Br2(g)
A Bit More Challenging…
6. The reaction
2 NO (g) ∏ N2 (g) + O2 (g)
has a value of Kc= 2400 at 2000 K. If 0.61 g of NO is put in a previously empty 3.00 L vessel,
calculate the equilibrium concentrations of NO, N2, and O2.
7. This equation is at equilibrium:
CO(g) + H2O (g) ↔ CO2 (g) + H2 (g)
If a 10.00L vessel has 2.50 mol CO2 and H2O, and 5.00 mol CO2 and H2 gas at 588 K, which way will
the reaction proceed? (Kc = 31.4 at 588°K)
What are the concentrations of all species at equilibrium?