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


84% (69 ratings)
View Complete Written Solution
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?

Frequently Asked Questions

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

Our tutors have indicated that to solve this problem you will need to apply the Activity Series concept. You can view video lessons to learn Activity Series. Or if you need more Activity Series practice, you can also practice Activity Series practice problems.