Problem: Consider the following unbalanced oxidation-reduction reactions in aqueous solution:Ag+(aq) + Li(s) → Ag(s) + Li+(aq)Fe(s) + Na+(aq) → Fe2+(aq) + Na(s)K(s) + H2O(l) → KOH(aq) + H2(g)Use the activity series to predict which of these reactions should occur. Are these results in accord with your conclusion in which of the reactions would you expect to be thermodynamically favored?

FREE Expert Solution

metals higher in the activity series are more reactive to oxidation and vice-versa.


I. Ag+(aq) + Li(s) → Ag(s) + Li+(aq)

Li higher in the activity series than Ag 

Li more reactive than Ag


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

Use the activity series to predict which of these reactions should occur. Are these results in accord with your conclusion in which of the reactions would you expect to be thermodynamically favored?

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What scientific concept do you need to know in order to solve this problem?

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