When is the reduction potential of a hydrogen | vedclass

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(A) The reduction reaction for a hydrogen half-cell is: $2H^+ (aq) + 2e^- \rightarrow H_2 (g)$.According to the Nernst equation,the reduction potentia

Vedclass · Accepted Answer

$p(H_2) = 2 \, atm$ and $[H^+] = 1.0 \, M$

Vedclass · Answer

(A) The reduction reaction for a hydrogen half-cell is: $2H^+ (aq) + 2e^- \rightarrow H_2 (g)$.According to the Nernst equation,the reduction potential $E_{H^+/H_2}$ is given by: $E = E^0 - \frac{0.0591}{2} \log \frac{p(H_2)}{[H^+]^2}$.Since $E^0 = 0 \, V$,the equation becomes: $E = -0.02955 \log \frac{p(H_2)}{[H^+]^2}$.For $E$ to be negative,$\log \frac{p(H_2)}{[H^+]^2}$ must be positive,which means $\frac{p(H_2)}{[H^+]^2} > 1$.Checking option $A$: $\frac{2}{(1.0)^2} = 2 > 1$. Thus,$E$ is negative.

When is the reduction potential of a hydrogen half-cell negative?

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