Consider the reaction A:H + B = B:H + A. If, at equilib- rium, the ratio of [B:H

Question

Consider the reaction A:H + B = B:H + A. If, at equilib- rium, the ratio of [B:H]/[B] is equal to 2.0, one can conclude that (1) B:H is the strongest reducing agent of the four com- pounds; (2) the (A:H-A) couple has a more negative redox potential than the (B:H-B) couple; (3) none of the four com- pounds are cytochromes; (4) the electrons associated with B are higher energy than those associated with A. Which of the pre- vious statements are true? Draw one of the half-reactions for this redox reaction.

Explanation / Answer

Statement (2) is the correct one.

At equilibrium, the reaction shifted more towards the right. That is A-H to A formation is more facile, when A- converts to A, it is oxidation. In the other half-reaction, B reduces to B-. So, the redox potential value of B/B- couple will be more than that of A/A- which means the redox potential value of A/A- couple will be more negative.

A-H = A- + H+

A- - e = A

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