Problem: The reaction A(g) ⇌  B(g) has an equilibrium constant of 5.8 and under certain conditions has Q = 336. What can you conclude about the sign of ΔG˚rxn and ΔGrxn for this reaction under these conditions?

🤓 Based on our data, we think this question is relevant for Professor Frantz's class at UVA.

FREE Expert Solution

Recall that when:

• Q > Ksp: the solution is supersaturated and a precipitate will form. Reactants are favored.

• Q = Ksp: the solution is at equilibrium and no precipitate will form.

• Q < Ksp: the solution is unsaturated and no precipitate will form. Products are favored. 


Our Q > K meaning we have a nonspontaneous reaction.

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Problem Details

The reaction A(g) ⇌  B(g) has an equilibrium constant of 5.8 and under certain conditions has Q = 336. What can you conclude about the sign of ΔG˚rxn and ΔGrxn for this reaction under these conditions?