E.m.f. of cell ${\rm{Ni}}\left| {{\rm{N}}{{\rm{i}}^{2 + }}\left( {0.1M} \right)} \right|\left| {{\rm{A}}{{\rm{u}}^{3 + }}\left( {1.0M} \right)} \right|{\rm{Au}}{\kern 1pt} {\kern 1pt} is \ldots ..,$ if ${E^ \circ }$ for ${\rm{N}}{{\rm{i}}^{2 + }}|{\rm{Ni}}$ is $ - 0.25{\rm{V}},{E^ \circ }$ for ${\rm{A}}{{\rm{u}}^{3 + }}|{\rm{Au}}$ is 1.50 V.

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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E.m.f. of cell

\mathrm{Ni}\left| {\mathrm{N}{\mathrm{i}^{2 + }}\left( {0.1M} \right)} \right|\left| {\mathrm{A}{\mathrm{u}^{3 + }}\left( {1.0M} \right)} \right|\mathrm{Au}{\kern 1pt} {\kern 1pt} is \ldots ..,

{E^ \circ }

for

\mathrm{N}{\mathrm{i}^{2 + }}|\mathrm{Ni}

- 0.25\mathrm{V},{E^ \circ }

for

\mathrm{A}{\mathrm{u}^{3 + }}|\mathrm{Au}

is 1.50 V.

View answer and explanation

Correct option: C

+ 1.75 V

Option C (+ 1.75 V) is correct because the EMF of the cell is calculated as the difference between the standard reduction potentials of the cathode and anode, with a correction for non-standard conditions using the Nernst equation.

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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