The anodic half-cell of lead-acid battery is recharged using electicity of 0.05 faraday .The amount of \mathrm{PbSO_{4}} electrolyzed in g during the process is _________

(Molar mass of \mathrm{PbSO_{4}=303g\, mol^{-1}})

Answers (1)

As we have learnt, 

When the anodic half of the lead storage battery is recharged, the following reaction occurs

 \mathrm{PbSO_4 + 2e^{-}\longrightarrow Pb +SO_4^{2-}}

Given that the total charge passed is \mathrm{0.05 ~F}

Now, from the balanced equation, it is clear that 

\mathrm{2~F} charge electrolyses \mathrm{1~mole} of \mathrm{PbSO_4}

\therefore \mathrm{0.05~F}charge electrolyses \mathrm{0.025 ~mole} of \mathrm{PbSO_4}

Thus, the mass of \mathrm{PbSO_4} electrolysed \mathrm{= 0.025 \times 303=7.575 ~g}

Therefore,option(3) is correct.

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