Problem: Consider the following unbalanced oxidation-reduction reactions in aqueous solution:l Ag+ (aq) + Li(s) → Ag(s) + Li+(aq)Fe(s) + Na+(aq) → Fe2+(aq) + Na(s)K(s) + H2O(l) → KOH(aq) + H2(g)Based on the values you obtain for ΔH˚, which of the reactions would you expect to be thermodynamically favored? (That is, which would you expect to be spontaneous?)

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A negative ΔH means the reaction is thermodynamically-favored (i.e. spontaneous).

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Problem Details
Consider the following unbalanced oxidation-reduction reactions in aqueous solution:
l Ag+ (aq) + Li(s) → Ag(s) + Li+(aq)
Fe(s) + Na+(aq) → Fe2+(aq) + Na(s)
K(s) + H2O(l) → KOH(aq) + H2(g)

Based on the values you obtain for ΔH˚, which of the reactions would you expect to be thermodynamically favored? (That is, which would you expect to be spontaneous?)

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