A 1.00 L flask containing the equilibrium mixture CO +Cl2 COCl2 was found to contain 0.400 mol of COCl2, 0.100 mol of CO, and 0.500 mol of Cl2. If 0.300 mol of CO is added at constant temperature, what will be the new concentrations of each component at equilibrium?(need quadratic)

Question

A 1.00 L flask containing the equilibrium mixture CO +Cl2 <-> COCl2 was found to contain 0.400 mol of COCl2, 0.100 mol of CO, and 0.500 mol of Cl2.  If 0.300 mol of CO is added at constant temperature, what will be the new concentrations of each component at equilibrium?(need quadratic)

DrBob222 · Answer

Kc = (COCl2)/(CO)(Cl2)
Substitute the equilibrium concns in the problem and solve for Kc. Then to part 2 of the problem.
...........CO + Cl2 ==> COCl2
initial...0.4...0.5.....0.4
change.....-x....-x......x
equil...0.4-x...0.50-x....x

Substitute from the ICE chart and solve for x, then evaluate CO, Cl2, COCl2
Post your work if you get stuck.