JEE MAIN - Chemistry (2019 - 9th January Morning Slot - No. 15)
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
Explanation
Pb(s) + SO$$_4^{ - 2}$$ $$ \to $$ PbSO4 + 2e$$-$$
$${{{n_{PbS{O_4}}}} \over 1} = {{{n_{e - }}} \over 2}$$
$$ \Rightarrow $$ $${{{n_{PbS{O_4}}}} \over 1} = {{0.05} \over 2}$$
$$ \therefore $$ Weight of PbSO4 $$=$$ $${{0.05} \over 2} \times 303 = 7.6g$$
$${{{n_{PbS{O_4}}}} \over 1} = {{{n_{e - }}} \over 2}$$
$$ \Rightarrow $$ $${{{n_{PbS{O_4}}}} \over 1} = {{0.05} \over 2}$$
$$ \therefore $$ Weight of PbSO4 $$=$$ $${{0.05} \over 2} \times 303 = 7.6g$$
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