Question: Use the References to access important values if needed for this question. At 351K and a total equilibrium pressure of 0.957 atm, the fractional dissociation

Use the References to access important values if needed for this

Use the References to access important values if needed for this question. At 351K and a total equilibrium pressure of 0.957 atm, the fractional dissociation of CH2Cl2 is 0.865 for the reaction 2CH2Cl2(g)?CH4(g)+CCl4(g) This means that 865 of every 1000 molecules of CH2Cl2 originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp=

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