1.At 800°C the value of Kp for NOCl(g) <-> NO(g)+ ½ Cl2(g) is 1.8×10-2. If a container is filled with NOCL(g) and allowed to reach equilibrium, the equilibrium pressure of NOCL(g ) and allowed to reach equilibrium, the equilibrium pressure of NOCL is 0.657atm. what are the equilibrium partial pressures of NO(g) and Cl2.
2.Suppose that 0.100atm each of the gases CO,H2,CO2 and H2O is placed in a container and allowed to come to equilibrium. Calculate the equilibrium pressure of all gases. (Kp=1.85) for the reaction CO(g)+H2O(g) <->H2(g)+CO2(g)
3.Initially pure NOCl gas was heated to 240°C in a 1.00L container. At equilibrium it was found that the total pressure was 1.00atm and the NOCl partial pressure was 0.64atm. 2NOCl(g)<->2NO(g)+Cl2(g). a.)calculate the partial pressures of NO and Cl2. (B.)calculate Kp.