Consider the equilibrium between COCl2, CO and Cl2. COCl2(g) CO(g) + Cl2(g) K = 0.142 at 920 K The reaction is allowed to reach equilibrium in a 8.00-L flask. At equilibrium, [COCl2] = 0.309 M, [CO] = 0.209 M and [Cl2] = 0.209 M. (a) The equilibrium mixture is transferred to a 16.0-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 16.0-L flask. [COCl2] M = [CO] M = [Cl2] M = If your equilibrium values are correct, when you substitute them into the equilibrium
Consider the equilibrium between COCl2, CO and Cl2.
COCl2(g) CO(g) + Cl2(g) K = 0.142 at 920 K
The reaction is allowed to reach equilibrium in a 8.00-L flask. At equilibrium, [COCl2] = 0.309 M, [CO] = 0.209 M and [Cl2] = 0.209 M.
(a) The equilibrium mixture is transferred to a 16.0-L flask. In which direction will the reaction proceed to reach equilibrium?
(b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 16.0-L flask.
[COCl2] M =
[CO] M =
[Cl2] M =
If your equilibrium values are correct, when you substitute them into the equilibrium expression you should reproduce the value of K given. please do this part last two times I asked they didn't and gave me the wrong answer
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