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# Equilibrium constant Kp

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Consider the following reaction:
CO2(g) + C(s) ----> 2CO(g)
At equilibrium, at a certain temperature, the partial pressures of CO2(g) and CO(g) are 33.7 and 9.26 atm, respectively. Calculate the value of Kp.

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Consider the following reaction:
CO2(g) + C(s)  2CO(g)
At equilibrium, at a certain temperature, the partial pressures of CO2(g) and CO(g) are 33.7 and 9.26 atm, respectively. Calculate the value of Kp.

When writing the Kp for a heterogeneous equilibrium, we don't need to include any term for a solid in the equilibrium expression.
So the expression of Kp is

This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!