Single Choice

The anodic half-cell of lead-acid battery is recharged unsing electricity of $$0.05$$ Faraday. The amount of $$PbSO_4$$ electrolyzed in g during the process is : $$($$ Molar mass of $$PbSO_4 = 303 g mol^{-1}) $$

A$$22.8$$
B$$15.2$$
C$$7.6$$
Correct Answer
D$$11.4$$

Solution

$$A)\ \underset{0.05/2\ mole}{PbSO_4}+2OH^- \rightarrow PbO_2 + H_2SO_4 +\underset{0.05F}{2e^-}$$ $$B)\ \underset{0.05/2\ mole}{PbSO_4 }+\underset{0.05\ F}{2e^-}+2H^+ \rightarrow Pb(s) + H_2SO_4$$ $$n_T(PbSO_4)=\dfrac{0.05}{2}\ mole$$ $$m_{PbSO_4}=\dfrac{0.05}{2}\times 303=7.6\ gm$$

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