# The anodic half -cell battery is recharged using  electicity of 0.05 faraday .The amount of $PbSO_{4}$ electrolyzwd in g during the process is ;(Molar mass of $PbSO_{4}=303g\, \, mol^{-1}$)Option 1)22.8Option 2)15.2Option 3)7.6Option 4)11.4

Reduction Half Reaction -

The half reaction that involve gain of electrons are called reduction half reaction.

- wherein

e.g. $Cl_{2}(g) + 2e^{^{-}}\rightarrow 2Cl^{-}(g)$

Oxidation Half Reaction -

Half reaction that involves loss of electrons are called oxidation half reactions

- wherein

e.g.$2Na (s)\rightarrow 2Na^{+}(g) + 2e^{-}$

Half Reaction Method -

1. Produce unbalanced equation for the reaction in ionic form.

2. Separate the equation into half reactions.

3. Balance the atoms other than O and H in each half reaction.

4. Add $H_{2}O$ to balance O atoms and $H^{+}$ to balance H atom.

5. Add electrons to one side of the half reaction to balance the charges.

as we know that $PbSO_{4}+2e^{-}\rightarrow Pb_{\left ( s \right )}+SO_{4}^{2-}$  when 2e-,2F current passed electrolyzed $PbSO_{4}$-=330gm/mol

so, 0.0f current passed  then electrolyzed$PbSO_{4}$ will  be =$\frac{303}{2\times 0.05}=7.6g$

Option 1)

22.8

Option 2)

15.2

Option 3)

7.6

Option 4)

11.4

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