The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of `PbSO_(4)` electrolyzed g during the process is: (Molar mass of `PbSO_(4) = gmol^(-1)`)

Options

A. `(11.4)`
B. `(15.2)`
C. `(22.8)`
D. `(7.6)`

Explanation

To solve the problem of how much PbSO₄ is electrolyzed when 0.05 Faraday of electricity is used, we can follow these steps:

### Step 1: Understand the Reaction
In the lead-acid battery, during the recharging process, lead sulfate (PbSO₄) is converted back to lead (Pb) and sulfate ions (SO₄²⁻) at the anode. The half-reaction can be represented as:
\[ \text{PbSO}_4 + 2e^- \rightarrow \text{Pb} + \text{SO}_4^{2-} \]

This indicates that 1 mole of PbSO₄ requires 2 moles of electrons (or 2 Faraday) for complete reduction.

...