🤓 Based on our data, we think this question is relevant for Professor Daykin's class at NCSU.
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
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:
We can use the following equation to solve for ΔG˚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.