Chemistry Equilibrium (Can Someone Answer This)

Question

The value of K_p for the equilibrium

COCl_2(g) <--> CO_(g) + Cl_2(g)

is 6.7 E^-4 at a certain temperature. If the initial partial pressure of COCl_2(g) is 0.87 atm

a. What will be the equilibrium partial pressures of COCl_2(g), CO_(g), Cl_2(g)

b. What will be the total pressure at equilibrium?

Answer 1

COCl_2(g)  <-===> CO_(g)  + Cl_2(g)

0.87........................0................0...........initial

-x...........................+x...............+x..........change

0.87-x.....................x..................x..........equillibrium

Kp = 6.7x10^-4 = (P_CO)(P_Cl2) / (P_COCl2) = (x)(x) / (0.87-x)

5.8x10-4 - 6.7x10-4x = x²

x² + 6.7x10-4x - 5.8x10-4 = 0

x = 0.024 atm

a) equilibrium partial pressures are as follows:

P_COCl2 = 0.87 - 0.024 = 0.846 = 0.85 atm

P_CO = 0.024 atm

P_Cl2 = 0.024 atm

b) Total pressure = sum of partial pressures = 0.85 + 0.024 + 0.024 = 0.894 = 0.89 atm