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?