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Topic: Partial Pressure  (Read 2298 times)

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Offline Violet89

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Partial Pressure
« on: March 03, 2013, 10:06:05 PM »
For the following reaction, Kp = 0.781 at a given temperature.

C(s) + 2 H2(g) <=> CH4(g)

At equilibrium, PCH4 = 3.82. What is the equilibrium partial pressure of H2?


0.781 = [3.82] / [C][H2]^2

Where do I go from here?


I'd appreciate any help.
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Offline Stovn0611

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Re: Partial Pressure
« Reply #1 on: March 03, 2013, 10:07:31 PM »
In a Kp expression, only partial pressures are included so carbon(solid) should not show up in the equilibrium expression.
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Offline Violet89

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Re: Partial Pressure
« Reply #2 on: March 03, 2013, 10:10:38 PM »
Quote from: Stovn0611 on March 03, 2013, 10:07:31 PM
In a Kp expression, only partial pressures are included so carbon(solid) should not show up in the equilibrium expression.

Thank you. I forgot about solids. So then the correct equation would be 0.781 = [3.82] / [H2]^2, which is equal to 2.21?
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