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This question asks if a reaction given reaction has multiple steps and the ratio of step 1's equilibrium constant to step 2's is 10/1, what is deltaG(step 2), given that deltaG(step 1) is -200kJ. The final answer is -194kJ. Since deltaG=-RTlnk and the only thing changing is lnk, I thought you could find the ratio of lnk/ln10k and just multiple -200 by this value. Why doesn't this work?
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