Recall that ΔG˚rxn and K are related to each other:
We can use the following equation to solve for ΔG˚rxn:
Step 1: We can use the following equation to solve for ΔH˚rxn:
Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol.
Also, note that ΔH˚f for elements in their standard state is 0.
We also need to convert ΔH˚rxn from kJ/mol to J/ mol so our units remain consistent.
ΔH˚rxn = –5.89 × 105 J/mol
Step 2: We can use the following equation to solve for ΔS˚rxn:
Note that we need to multiply each S˚ by the stoichiometric coefficient since S˚ is in J/mol • K.
ΔS˚rxn = –498.18 J/mol • K
Step 3: Now that we have ΔH˚rxn and ΔS˚rxn, we can now solve for ΔG˚rxn.
The given temperature is 298 K.
ΔG˚rxn = –440542.36 J/mol
Step 4: Solving for K:
Use data from Appendix IIB in the textbook to calculate the equilibrium constants at 25 ˚C for each of the following reactions.
2 CO(g) + O2(g) ⇌ 2 CO2(g)
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