Problem: Consider the following reaction: CH3OH(g) ⇌ CO(g) + 2H2 (g) Calculate ΔG for this reaction at 25°C under the following conditions: PCH3OH = 0.890 atm PCO = 0.120 atm PH2 = 0.200 atm Δ G =                           kJ

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We’re being asked to determine the standard free energy change (ΔG) at 25 ˚C for the given reaction:

CH3OH(g)  CO(g) + 2 H2(g)


Because of the double-arrows, we can say that this is an equilibrium reaction. 


We are given the following equilibrium pressures of each compound:

PCH3OH = 0.890 atm

PCO = 0.120 atm

PH2 = 0.200 atm


Recall that ΔG and K are related to each other:


ΔG°rxn=-RTlnK


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Problem Details

Consider the following reaction: 

CH3OH(g) ⇌ CO(g) + 2H2 (g) 

Calculate ΔG for this reaction at 25°C under the following conditions: 

PCH3OH = 0.890 atm 

PCO = 0.120 atm 

PH2 = 0.200 atm 

Δ G =                           kJ

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