We're being asked to determine the K or equilibrium constant for a reaction with ΔG° (standard free energy) for the reaction:
We can use the following equation to solve for ΔG˚rxn:
Note that we need to multiply each ΔG˚f by the stoichiometric coefficient since ΔG˚f is in kJ/mol.
ΔG˚rxn = –32.8 kJ
Now use the ΔG°-K equation where:
where ΔG is the free energy in J/mol K;
R is the gas constant (8.314 J/molK);
T is temperature in K;
and K as equilibrium constant
Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for this reaction: N2(g)+3H2(g)⇌2NH3(g)
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