Question

Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl, is allowed to dissociate into CO and Cl, at 873 K. At equilibrium, [COCI2] = 0.184 M, and [CO] = [Cl2] = 0.113 M. Additional CO is added so that (CO)new = 0.175 M and the system is allowed to once again reach equilibrium. K= COC12(g) CO(g) + Cl2(g) 6.98x10-2 at 873 K (a) In which direction will the reaction proceed to reach equilibrium? (b) What are the new concentrations of reactants and products after the system reaches equilibrium? M [COCI2] = C [CO] = [Cl2] =D

Answer 1

(a) In which direction will the reaction proceed to reach equilibrium? : backwards direction or to the left towards the reactants.

(b) [COCl₂] = 0.205 M

[CO] = 0.154 M

[Cl₂] = 0.0924 M

Explanation

initial concentration COCl₂ = 0.184 M

initial concentration CO = 0.175 M

initial concentration Cl₂ = 0.113 M

equilibrium constant K = 6.98 x 10^-2

ICE table	COCl2 (g)	$\rightleftharpoons$	CO (g)	Cl2 (g)
Initial conc.	0.184 M		0.175 M	0.113 M
Change	-x		+x	+x
Equilibrium conc.	0.184 M - x		0.175 M + x	0.113 M + x

K = [CO]_eq[Cl₂]_eq / [COCl₂]_eq

6.98 x 10^-2 = [(0.175 M + x) * (0.113 M + x)] / (0.184 M - x)

Solving for x, x = -0.02055 M

equilibrium concentration COCl₂ = 0.184 M - x

equilibrium concentration COCl₂ = 0.184 M - (-0.02055 M)

equilibrium concentration COCl₂ = 0.205 M

equilibrium concentration CO = 0.175 M + x

equilibrium concentration CO = 0.175 M + (-0.02055 M)

equilibrium concentration CO = 0.154 M