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.
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?
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