rank the following reactions from smallest to largest equilibrium constant (K) at 298K?reaction 1: Fe2O3(s)+3CO(g)->2Fe(s)+3CO2(g), ∆G°=-28.0kJreaction 2: Ca CO3(s)->CaO(s)+CO2(g), ∆G°=+131.1kJreaction 3: 2Hg(g)+O2(g)->2HgO(s), ∆G°=-180.8kJreaction 4: 3O2(g)->2O3(g), ∆G°=+326kJthe answer is suppose to be (reaction 1, reaction 3, reaction 2, reaction 4) but I don't understand how this is possible.I was told to use Keq=e^-∆G° / RT. The values I got for the reaction are: 1.0113, 0.94846, 1.0757 and 0.87671, but I don't know how 1.0113<1.0757<0.94846< 0.87671

Keq = e^(-∆G° / RT) We know, ∆G<0, then the reaction is spontaneous and Keq is high and, if…

Answered: rank the following reactions from…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 16P

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rank the following reactions from smallest to largest equilibrium constant (K) at 298K?

reaction 1: Fe₂O₃(s)+3CO(g)->2Fe(s)+3CO₂(g), ∆G°=-28.0kJ

reaction 2: Ca CO₃(s)->CaO(s)+CO₂(g), ∆G°=+131.1kJ

reaction 3: 2Hg(g)+O₂(g)->2HgO(s), ∆G°=-180.8kJ

reaction 4: 3O₂(g)->2O₃(g), ∆G°=+326kJ

the answer is suppose to be (reaction 1, reaction 3, reaction 2, reaction 4) but I don't understand how this is possible.

I was told to use Keq=e^-∆G° / RT. The values I got for the reaction are: 1.0113, 0.94846, 1.0757 and 0.87671, but I don't know how 1.0113<1.0757<0.94846< 0.87671

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