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October 26, 2014

October 26, 2014

Posted by **Chem** on Saturday, November 17, 2007 at 1:06pm.

At 25Â°C (delta)Ho = -92.22 kJ and (delta)So = -198.53 J/K. Using this information, calculate the equilibrium constant for the reaction at 2.43x10^2Â°C. (R = 8.314 J/K)

Apparently the way I'm doing it is wrong:

I divide 198.53 by 1000 then multiply by 298 to get delta(S). Then I subtract this from delta(H) to get delta(G). Then I multiply 516 with .008314... I take this answer and divide delta(G) by it, then multiply by -1. I take this to the e power... Then I use the equation Kc = (RT)^-n * Kp to get the equilibrium constant. However my answer is still wrong.

- Dan -
**DrBob222**, Saturday, November 17, 2007 at 1:33pmor mike or whomever,

Two points:

1. How do you know to calculate Kc instead of Kp? The problem doesn't specify which. Since this is a gaseous reaction, Kp may be what they are looking for.

2. Have you tried the van't Hoff equation. You have delta H and one T so the van't Hoff equation can be used to calculate K at any other T.

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