The equilibrium constant, Kp, for the following reaction is 0.636 at 600K. COCl2(g) <=> CO(g) + Cl2(g)

If an equilibrium mixture of the three gases in a 16.9 L container at 600K contains COCl2 at a pressure of 0.836 atm and CO at a pressure of 0.551 atm, the equilibrium partial pressure of Cl2 is atm.

The equilibrium partial pressure of is 0.964 atm.

Explanation:

Given:

The given reaction equation is as follows.

Formula used to calculate the partial pressure of is as follows.

Substitute the values into above formula as follows.

Thus, we can conclude that the equilibrium partial pressure of is 0.964 atm.

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