1. Calculate the equilibrium constant, Keq, for the following reaction at 25 C, if [NO]eq = 0.106 M, [02]eq = 0.122 M and [NO2]eq = 0.129 M. 2 NO (g) + O2 (g) 2 NO2 (g) 2. Find the equilibrium constant, Keq, for the following equilibrium. The initial concentrations of AB and A2D are 0.30 M before they are mixed and when equilibrium is reached, the equilibrium concentration of A2D is 0.20 M. Use an ICE table for your calculation. 2 AB (g) + CD (s) AD (g) +2 CB (s) If 0.50 mol of NO2 is placed in a 2.0L flask to create NO and O2, calculate []eq if Keq = 1.2 x 10-5. (Answer: [02]eq = 0.0057 M, [NO]eq = 0.0114 M, [NO2] eq = 0.24 M). For the system, if we start with 0.100mol/L of CO2 and H2, what are the concentrations of the reactants and products at equilibrium given that Keq = 0.64 at 900K? CO2 (g) + H2 (g) Co (g) + H2O (g) 4. For the system, if we start with 0.010 mol/L of H2 and 12 and 0.096 mol/L of HI, what are their concentrations at equilibrium given that Keq = 0.016? H2 + 12 2HI 5. At 650C, the reaction below has a Keq value of 0.771. If 2.00 mol of both hydrogen and carbon dioxide are placed in a 4.00 L container and allowed to react, what will be the equilibrium concentrations of all four gases? H2 (g)+ CO2 (g) CO (g) + H2O (g) 6. Carbonyl bromide, COBr2, can be formed by reacting CO with Br2. A mixture of 0.400 mol CO, 0.300 mol Br2, and 0.0200 mol COBr2 is sealed in a 5.00L flask. Calculate equilibrium concentrations for all gases, given that the Keq = 0.680. CO (g) + Br2 (g) COBr2 (g)