The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) CCl4(g) Calculate the equilibrium partial pressures of

The complete question is as follows: The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.968 atm at 350 K. PCH2Cl2 = atm PCH4 = atm PCCl4 = atm

The equilibrium partial pressures of all species, that is, , and is 0.420 atm, 0.420 atm and 0.128 atm.

Explanation:

For the given reaction equation, the initial and equilibrium concentration of involved species is as follows.

Initial:                0.968 atm         0               0

Equilibrium:  (0.968 - 2x)           x                x

Now, for this reaction is as follows.

Thus, we can conclude that the equilibrium partial pressures of all species, that is, , and is 0.420 atm, 0.420 atm and 0.128 atm.

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