Calculate the quantity of electricity ( in Faraday) that would be required to reduce 12.3 g of nitrobenzene to aniline, if current efficiency is 50% (write answer in nearest integer).

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Solution

$C_{6} H_{5} N O_{2} + 6 H^{+} + 6 e \to C_{6} H_{5} N H_{2} + 2 H_{2} O$
or $N^{3 +} + 6 e \to N^{3 -}$

$∴$ Eq. mass of nitrobenzene $= \frac{M}{6} = \frac{123}{6}$
Now $m = \frac{E \times i \times t}{96500}$

$12.3 = \frac{123 \times i \times 50 \times t}{6 \times 100 \times 96500}$

$i \times t = 1.2 \times 96500$ C $= 1.2$ F

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Calculate the quantity of electricity ( in Faraday) that would be required to reduce 12.3 g of nitrobenzene to aniline, if current efficiency is 50% (write answer in nearest integer).

C6H5NO2+6H++6e→C6H5NH2+2H2Oor N3++6e→N3−∴ Eq. mass of nitrobenzene =M6=1236Now m=E×i×t9650012.3=123×i×50×t6×100×96500i×t=1.2×96500 C =1.2 F