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?)
FREE Expert Solution
A negative ΔH means the reaction is thermodynamically-favored (i.e. spontaneous).
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)
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?)
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 Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.