CHEMISTRY COMMUNITY

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?

Please include a photo of the question since most students will only have the previous final exams starting at 2011 in their course readers.

Attached is a photo of the problem