For the following reaction, K c = 255 at 1000 K. CO (g) + Cl2 (g) ? COCl2 (g) A

Question

For the following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) ? COCl2 (g)
A reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.172 M at 1000 K.

Part A

What is the equilibrium concentration of CO at 1000 K?

Express your answer in molarity to three significant figures.

Part B

What is the equilibrium concentration of Cl2 at 1000 K?

Express your answer in molarity to three significant figures.

[Cl2] =? M

Part C

What is the equilibrium concentration of COCl2 at 1000 K?

Express your answer in molarity to three significant figures

[COCl2] =? M

Explanation / Answer

CO(g) + Cl?(g) ? COCl?(g)
the equilibrium concentrations in M are related as:
Kc = [COCl?] / ( [CO]?[Cl?] )
with Kc = 255

ICE-Table
........... [CO]......... [Cl?].......... [COCl?]
I.......... 0.155....... 0.176............. 0
C........... -x............ -x...............+x
E....... 0.155 -x.... 0.176-x.......... x

When you substitute the expressions for the equilibrium concentrations from the last row of the table to the equilibrium equation you get:
255 = x / ( (0.155 - x)?(0.176 - x))
<=>
255? (0.155 - x)?(0.176 - x) = x
<=>
255?(0.02728 - 0.331?x + x

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