Question

Suppose reaction X has a reduction potential of -0.311 V, while reaction Y has a reduction potential of -0.109 V. Which reaction is more likely to run backwards as an oxidation? Group of answer choices

a. Both are equally likely
b. Reaction Y
c. Reaction X

Answer 1

Reaction Y, with a standard reduction potential of -0.109 V, is more likely to run backwards as an oxidation compared to Reaction X with a standard reduction potential of -0.311 V, given that Y's potential is less negative.

Step-by-step explanation:

The likelihood of a reaction to run backwards as an oxidation is higher for the reaction with the less negative (or more positive) standard reduction potential. In this case, Reaction Y has a reduction potential of -0.109 V, which is less negative than Reaction X's reduction potential of -0.311 V. Therefore, Reaction Y is more likely to run backwards as an oxidation, as its potential is closer to being positive.

By reversing the reduction reaction to get the oxidation potential, the sign of the reduction potential changes. The more positive the oxidation potential, the more likely the reaction is to occur in the forward direction as an oxidation process. According to standard reduction potentials, Reaction Y is deemed to have a more positive oxidation potential than Reaction X when run in reverse, indicating Reaction Y is more predisposed to oxidation.