O2M(s) —-> M(s) +O2(g) delta G= 288.9 Kj/mol

When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s).

I got an answer of :

O2M(s)+ C(s) —-> M(s) + CO2(g)

This is correct. I need help on this part of the question:

What is the thermodynamic equilbrium constant for the coupled reaction?

I attempted this twice and got

K=1.22 and 0.89 and they are both wrong. Please help.

(105,500/8.314*298) = lnK and i get a huge number for K. Somethng like 3.1E18

Check that carefully.

i got K=1.69e18 as my answer and it was correct.

still getting the equation wrong though :/

2:Find thr delta g for the gases.

3:Find the delta g for the second equation.

4:Add the delta g’s for the 2 questions together.

5: Solve for the value of Q using the equation

-Delta G not =RTLnQ

deltaG(system)=deltaG[CO2]+deltaG[M]-deltaG[MO2]-deltaG[C]

look up deltaG value from table for CO2=-394.4

DeltaG for a solid is almost always zero (C)

So -394.4+288.9=deltaGsystem

then

K=e^((deltaGsystem)/((8.314/1000)*298)))

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