2. Calculating Kp from equilibrium amounts (a)In the following reaction: CO2 (g) + H2 (g)  CO (g) + H2O (g)
at a temperature of and a pressure of 2.0 atm, the amounts of each gas present at equilibrium were 6.2 x 10-3 mol of CO, 6.2 x 10-3 mol of H2O, 0.994 mol of CO2
and 0.994 mol of H2. Calculate the value of Kp.
(b)In the following reaction: H2 (g) + I2 (g)  2HI (g)
at a temperature of 485C and a pressure of 2.00 atm, the amount of each gas present was 0.56 mol of H2, 0.06 mol of I2 and 1.27 mol of HI. Calculate Kp at this temperature.

3. Calculating pressure from Kp and equilibrium amounts
(a)In the following reaction: 2NO2 (g)  2NO (g) + O2 (g)
at a temperature of 700K, the amount of each gas present at equilibrium is 0.96 mol of NO2, 0.04 mol of NO and 0.02 mol of O2 . If Kp = 6.8 x 10-6 atm what must the total pressure have been to obtain this particular equilibrium mixture?
(b)Kp = 3.72 atm at 1000K for the system: C (s) + H2O (g)  CO (g) + H2 (g)
What pressure must be applied to obtain a mixture containing 2.0 mol of CO,
1.0 mol of H2 and 4.0 mol of H2O?

4. Calculating Kp from percentage dissociation
(a)When the following equilibrium was established at a given temperature 20% of the compound A2B2 was dissociated. The total pressure of the equilibrium mixture was 30 atm. Calculate the value of Kp at this temperature. A2B2 (g)  2AB (g)
(b)When the following equilibrium was established at a given temperature 75% of the sulphur trioxide was dissociated. The total pressure of the equilibrium mixture was 10 atm. Calculate the value of Kp at this temperature. 2SO3 (g)  2SO2 (g) + O2 (g)