- A$3$
- B$5$
- C$6$
- D$4$
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For the cell $\mathrm{Cu}(\mathrm{s})\left|\mathrm{Cu}^{2+}(\mathrm{aq})(0.01 \mathrm{M}) \| \mathrm{Ag}^{+}(\mathrm{aq})(0.001 \mathrm{M})\right| \mathrm{Ag}(\mathrm{s})$ the cell potential $=.....\times 10^{-2} \mathrm{~V}$
(Round off to the Nearest Integer).
[Use: $\frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059$ ]

$MnCl _2+ K _2 S _2 O _8+ H _2 O \longrightarrow KMnO _4+ H _2 SO _4+ HCl$ (equation not balanced).
Few drops of concentrated $HCl$ were added to this solution and gently warmed. Further, oxalic acid ( $225 mg$ ) was added in portions till the colour of the permanganate ion disappeared. The quantity of $MnCl _2$ (in $mg$ ) present in the initial solution is. . . . . . . . . (Atomic weights in $g mol ^{-1}: Mn =55, Cl =35.5$ )