Question:
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 in : (Molar mass of $ {PbSO_4 = 303 \; g \; mol^{-1}}$)
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 in : (Molar mass of $ {PbSO_4 = 303 \; g \; mol^{-1}}$)
Updated On: Sep 14, 2024
- 22.8
- 15.2
- 7.6
- 11.4
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The Correct Option is B
Solution and Explanation
(A) $ { $\underset{\text{ 0.05/2 mole}}{ { PbSO4(s) }}$ + 2OH^{-} -> PbO_2 + H2SO4 + $\underset{\text{ 0.05F}}{ { 2e^{-}}}$ }$
(C) $ { $\underset{\text{ 0.05/2 mole 0.05 F}}{ { PbSO4 + 2e^{-}}}$ + 2H^{+} -> Pb(s) + H2SO4}$
$ { n_{T} (PbSO_4) = 0.05 \, mole} $
$ {m_{PbSO_{4}} = 0.05 \times 303 = 15.2 \; gm }$
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Concepts Used:
Nernst Equation
This equation relates the equilibrium cell potential (also called the Nernst potential) to its concentration gradient across a membrane. If there is a concentration gradient for the ion across the membrane, an electric potential will form, and if selective ion channels exist the ion can cross the membrane.
