The potential of the following cell is 0.34 V at ${25^ \circ }C$. Calculate the standard reduction potential of the copper half-cell. ${\rm{Pt}}\left| {{{\rm{H}}_2}\left( {1{\kern 1pt} {\kern 1pt} {\rm{atm}}} \right)} \right|{{\rm{H}}^ + }\left( {1{\rm{M}}} \right)|\left| {{\rm{C}}{{\rm{u}}^{2 + }}\left( {1{\rm{M}}} \right)} \right|{\rm{Cu}}$

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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The potential of the following cell is 0.34 V at

{25^ \circ }C

. Calculate the standard reduction potential of the copper half-cell.

\mathrm{Pt}\left| {{\mathrm{H}_2}\left( {1{\kern 1pt} {\kern 1pt} \mathrm{atm}} \right)} \right|{\mathrm{H}^ + }\left( {1\mathrm{M}} \right)|\left| {\mathrm{C}{\mathrm{u}^{2 + }}\left( {1\mathrm{M}} \right)} \right|\mathrm{Cu}

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Correct option: D

+0.34 V

Option D (+0.34 V) is correct because the standard reduction potential of the hydrogen electrode is 0 V, so the cell potential equals the copper half-cell potential.

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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