# 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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###### FREE Expert Solution

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:

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

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

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{-}}{\mathbf{T\Delta S}}{{\mathbf{°}}}_{{\mathbf{rxn}}}}$

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.

81% (277 ratings)
###### 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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

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Based on our data, we think this problem is relevant for Professor Daykin's class at NCSU.