Chemistry Gibbs Free Energy Solution: At 1500°C the equilibrium constant for the reactio...

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Solution: 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

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/mol
b) 233 kJ/mol
c) -105 kJ/mol
d) 105/mol
e) 1.07 kJ/mol

Solution

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:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

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