What is the reduction potential of a hydrogen | vedclass

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(B) The reduction half-reaction for the hydrogen electrode is: $2H^+ (aq) + 2e^- \rightarrow H_2 (g)$.According to the Nernst equation at $298 \ K$:$E

Vedclass · Accepted Answer

$-0.0592$

Vedclass · Answer

(B) The reduction half-reaction for the hydrogen electrode is: $2H^+ (aq) + 2e^- ightarrow H_2 (g)$.According to the Nernst equation at $298 \ K$:$E_{red} = E^\circ_{red} - \frac{0.0591}{n} \log \frac{P_{H_2}}{[H^+]^2}$.Given $E^\circ_{red} = 0 \ V$,$P_{H_2} = 1 \ atm$,$n = 2$,and $pH = 1$ (which means $[H^+] = 10^{-1} \ M$):$E_{red} = 0 - \frac{0.0591}{2} \log \frac{1}{(10^{-1})^2}$.$E_{red} = -0.02955 	imes \log(10^2) = -0.02955 	imes 2 = -0.0591 \ V$.Rounding to the nearest option,the value is $-0.0592 \ V$.

What is the reduction potential of a hydrogen gas electrode when pure hydrogen gas is at $1 \ atm$ pressure and the platinum electrode is in contact with an $HCl$ solution of $pH$ $1$ at $298 \ K$ (in $V$)?

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