Explanation

(d)
Given, mass of nitrobenzene = 12.3 g
Molecular mass of nitrobenzene = 123 g
∴ $Moles\ = \ \frac{12.3}{123}\ = 0.1\$
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∴ $H_{2}\$required for reduction of 0.1 mole nitrobenzene
$= \ 0.1\ \times \ 3\ = \ 0.3\ mol\ of\ hydrogen$
∴ Amount of charge required to liberate 0.3 mol of hydrogen
$= \ 2\ \times \ 96500\ \times \ 0.3\ (\because\ H_{2}\ \longrightarrow \ {2H}^{+})$
= 57900 C