The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO4 electrolyzed in g during the process is: (Molar mass of PbSO4 = 303 g mol

Engineering

Chemistry

Batteries and Fuel Cell

Question

The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO₄ electrolyzed in g during the process is: (Molar mass of PbSO₄ = 303 g mol^–1)

22.8

15.2

7.6

11.4

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$Pb (s) + {SO}_{4}^{2 -} \overset{}{\to} {PbSO}_{4} + 2 e^{-}$

For 2F current passed, PbSO₄ deposited = 303 g/mol

For 0.05 F: PbSO₄ deposited $= \frac{0 .05 \times 303}{2} = 7 .6 g$