Problem: At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) ⇌ CH3OH(g) has the value Kp = 1.4 x 10-7. Calculate ΔGº  for this reaction at 1500°C.a) -233 kJ/molb) 233 kJ/molc) -105 kJ/mold) 105/mole) 1.07 kJ/mol

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We’re being asked to determine the standard free energy change (ΔG) at 1500 ˚C for the given reaction:

CO2(g) + 2 H2(g)  CH3OH(g)


Recall that ΔG and K are related to each other:


ΔG°rxn=-RTlnK


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Problem Details

At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) ⇌ CH3OH(g) has the value Kp = 1.4 x 10-7. Calculate ΔGº  for this reaction at 1500°C.

a) -233 kJ/mol

b) 233 kJ/mol

c) -105 kJ/mol

d) 105/mol

e) 1.07 kJ/mol



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