The standard reduction potential ${E^ \circ }$ for the half reactions are as ${\rm{Zn}} \to {\rm{Z}}{{\rm{n}}^{2 + }} + 2{e^ - },{E^ \circ } = 0.76V$ ${\rm{Cu}} \to {\rm{C}}{{\rm{u}}^{2 + }} + 2{e^ - },{E^ \circ } = 0.34V$ The emf for the cell reaction, ${\rm{Zn}} + {\rm{C}}{{\rm{u}}^{2 + }} \to {\rm{Z}}{{\rm{n}}^{2 + }} + {\rm{Cu}}$

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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The standard reduction potential 

{E^ \circ }

for the half reactions are as

\mathrm{Zn} \to \mathrm{Z}{\mathrm{n}^{2 + }} + 2{e^ - },{E^ \circ } = 0.76V

\mathrm{Cu} \to \mathrm{C}{\mathrm{u}^{2 + }} + 2{e^ - },{E^ \circ } = 0.34V

The emf for the cell reaction,

\mathrm{Zn} + \mathrm{C}{\mathrm{u}^{2 + }} \to \mathrm{Z}{\mathrm{n}^{2 + }} + \mathrm{Cu}

View answer and explanation

Correct option: A

0.42 V

Option A (0.42 V) is correct because it is the cell potential calculated by subtracting the oxidation potential of copper from the oxidation potential of zinc.

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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