For the following reaction, Kc = 255 at 1000K. CO(g) + Cl 2 (g) COCl 2 (g) A rea

Question

For the following reaction, Kc = 255 at 1000K.

CO(g) + Cl2(g) COCl2(g)

A reaction mixture initially contains a CO concentration of 0.1530M and a Cl2 concentration of 0.179M at 1000K.

What is the equilibrium concentration of CO at 1000 K?

What is the equilibrium concentration of Cl2 at 1000 K?

What is the equilibrium concentration of COCl2 at 1000 K?

I attempted to follow a similar problem but cannot understand it. I also mess up on setting up the whole ICE chart. Can you make sure that my ice chart is right and explain how to do this? Thanks in advance!

Explanation / Answer

ICE table

                               CO           +             Cl2           ------------>         COCl2

initial                     0.1530                    0.179                                       0

change                   -x                             -x                                          +x

equilibrium          0.1530-x                 0.179-x                                      x

Feed values in Kc equation,

Kc = 255 = (x)/(0.1530-x)(0.179-x)

255(0.0274 - 0.332x + x^2) = x

6.987 - 74.7x + 255x^2 = x

255x^2 - 75.7x + 6.987 = 0

x = 0.148 M

So, equilibrium concentration of,

[CO] = 0.1530 - 0.148 = 0.005 M

[Cl2] = 0.179 - 0.148 = 0.031 M

[COCl2] = 0.148 M

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