Name:_____________________________ Date:_____________ Period:____
WS Equilibrium Calculations Practice III (with x’s)
H2O(g) + Cl2O(g) ↔ 2 HOCl(g)
Kc = 0.676
1. 1.0 mol pure HOCl is placed in a 2.0 L flask. Calculate the equilibrium concentrations of
H2O(g) and Cl2O(g).
2.
Gaseous HCl is added to a rigid vessel containing excess solid iodine at 25oC until the partial
pressure of HCl reaches 1.47 atm. The following reaction brings the system to equilibrium.
2 HCl(g) + I2(s) ↔ 2 HI(g) + Cl2(g)
Kp = 3.91 x 10–33 at 25oC
(a) Find the equilibrium partial pressures of all species at 25oC.
The temperature of the system changed so that the equilibrium constant, Kp , is 8.39 x 10–27.
(b) Find the new partial pressures of all the species at equilibrium.
HCl(g) + CH3Cl(g) ↔ CH4(g) + Cl2(g)
3.
The equilibrium constant, Kp , is 6.3 x 10–15 at 1500 K for the reaction represented above. A
chemist mixes 45.0% HCl(g) and 55.0% CH3Cl(g) by moles into a container so that the total
pressure inside the container is 1.50 atm at 1500 K.
(a) Find the initial pressures of each gas.
(b) Find the equilibrium partial pressures of each gas at 1500 K.
HCl(g) + CH3Cl(g) ↔ CH4(g) + Cl2(g)
The temperature of the system changed so that the equilibrium constant, Kp , is 4.7 x 10–10.
(c) Find the new partial pressures of all gaseous species at equilibrium.