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At 365 K and a total equilibrium pressure of 0.985 atm, the fractional dissociation of CH2Cl2...

At 365 K and a total equilibrium pressure of 0.985 atm, the fractional dissociation of CH2Cl2 is 0.850 for the reaction

2CH2Cl2(g) <----> CH4(g) + CCl4(g)

This means that 850 of every 1000 molecules of CH2Cl2 originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp.

Kp = _______

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