Given below are half-cell reactions:

\(\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \\ \mathrm{E}_{\mathrm{Mn}^{2+}}^{\circ} / \mathrm{MnO}_{4}^{-}=-1.510 \mathrm{~V} \\ \frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}, \\ \mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\circ}=+1.223 \mathrm{~V}\)

Will the permanganate ion, \(\mathrm{MnO}_{4}^{-}\) , liberate \(\mathrm{O}_{2}\) from water in the presence of an acid?

1. No, because \(\mathrm{E}_{\text {cell }}^{\circ}=-2.733 \mathrm{~V}\)
2. Yes, because \(\mathrm{E}_{\text {cell }}^{\circ}=+0.287 \mathrm{~V}\)
3. No, because \(\mathrm{E}_{\text {cell }}^{\circ}=-0.287 \mathrm{~V}\)
4. Yes, because \(\mathrm{E}_{\text {cell }}^{\circ}=+2.733 \mathrm{~V}\)
Subtopic:  Electrode & Electrode Potential |
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Two half cell reactions are given below :
\(\begin{aligned} &\mathrm{Co}^{3+}+e^{-} \rightarrow \mathrm{Co}^{2+}, \mathrm{E}_{\mathrm{Co}^{2+} / \mathrm{Co}^{3+}}^{\circ}=-1.81 \mathrm{~V} \\ &2 \mathrm{Al}^{3+}+6 e^{-} \rightarrow 2 \mathrm{Al}(\mathrm{s}), \mathrm{E}_{\mathrm{Al} / \mathrm{Al}^{3+}}^{\circ}=+1.66 \mathrm{~V} \end{aligned} \)
The standard EMF of a cell with feasible redox reaction will be:
1. +7.09 V
2. +0.15 V
3. +3.47 V
4. –3.47 V

Subtopic:  Electrode & Electrode Potential |
To view explanation, please take trial in the course below.
NEET 2023 - Target Batch - Aryan Raj Singh
To view explanation, please take trial in the course below.
NEET 2023 - Target Batch - Aryan Raj Singh
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