Question 1: (Multiple Parts)

a) 2 AB(g) + C2D(s) A2D(g) + 2 CB(s)

Find the equilibrium constant, Kc, for the following equilibrium. The initial concentrations of AB and A2D are 0.30 M before they are mixed. When equilibrium is reached, the equilibrium concentration of A2D is 0.20 M. Express your answer to the correct number of sig figs. Kc is unitless.

b)H2S(g) H2(g) + S(g)

At a certain temperature, the Kp for the decomposition of H2S is 0.723. Initially, only H2S is present at a pressure of 0.165 atm in a closed container. What is the total pressure in the container at equilibrium? Express your answer to the correct number of sig figs and do not include units. (Hint: don't round until the end, Dalton's law of partial pressures will help!)

c) CO(g) + H2O(g) CO2(g) + H2(g)

At a particular temperature, 0.492 M H2 and 0.492 M CO2 gases were added to a sealed reaction vessel and allowed to react to equilibrium. If the equilibrium constant, Kc, for this reaction is 1.5, what is the equilibrium concentration (M) of CO? Express your answer to the correct number of sig figs and do not include units.

d) __ NO2(g) __ NO(g) + __ O2(g)

If 0.50 mol of NO2 is placed in a sealed 2.0 L flask and allowed to decompose to NO and O2 according to the following unbalanced equation, calculate the equilibrium concentration (M) of NO if Kc = 1.2 105. Express your answer to the correct number of sig figs and do not include units.

e) CO(g) + Br2(g) COBr2(g)

Carbonyl bromide, COBr2, can be formed by reacting CO with Br2 according to the following reaction. A mixture of 0.400 mol CO, 0.300 mol Br2, and 0.0200 mol COBr2 is sealed in a 5.00 L flask. Calculate the equilibrium concentration of COBr2 (M), given that Kc = 0.680. Express your answer to the correct number of sig figs and do not include units.