Problem: Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0º C. H2 (g) + CO2 (g) ⇌ CO (g) + H2O (g)Δ Hº = 41.15 kJΔ Sº = 42.35 J/K 

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We’re being asked to determine the equilibrium constant (K) at 25 ˚C for the given reaction:

H2(g) + CO2(g)  CO(g) + H2O(g)


Recall that ΔG˚rxn and K are related to each other:


ΔG°rxn=-RTlnK


We can use the following equation to solve for ΔG˚rxn:


ΔG°rxn=ΔH°rxn-TΔS°rxn


We’re given the ΔH˚rxn and ΔS˚rxn of the reaction:

ΔH˚rxn = 41.15 kJ

ΔS˚rxn = 42.35 J/K


For this problem, we need to do the following steps:

Step 1: Use ΔH˚rxn and ΔS˚rxn to calculate for ΔG˚rxn.

Step 2: Calculate for K.


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Problem Details

Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0º C.

 H2 (g) + CO2 (g) ⇌ CO (g) + H2O (g)

Δ Hº = 41.15 kJ
Δ Sº = 42.35 J/K 

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