While charging the lead storage battery

Question

While charging the lead storage battery (A) PbSO4 on anode is reduced to Pb (B) PbSO4 on cathode is reduced to Pb (C) PbSO4 on cathode is oxidized to Pb (D) PbSO4 on anode is oxidized to PbO2

Tardigrade Admin · Accepted Answer

Lead-acid batteries, also known as lead storage batteries, can store a lot of charge and provide high current for short periods of time.
Lead-acid batteries are capable of being recharged, which is important for their use in cars.

This type of battery can be recharged. In the charged state, each cell contains negative plates of elemental lead

(P b)

and positive plates of lead(IV) oxide

(P b O_{2})

in an electrolyte of approximately

4.2 M

sulfuric acid

(H_{2} S O_{4})

. The charging process is driven by the forcible removal of electrons from the positive plate and the forcible introduction of them to the negative plate by the charging source.
The charging equation is,

< b r / > 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)} \to P b_{(s)} + P b O_{2 (s)} + 2 H_{(a q)}^{+} + 2 H S O_{4 (a q)}^{-} < b r / >

On charging the battery the reaction is reversed and

P b S O_{4 (s)}

is converted into

P b

at anode and

P b O_{2}

at cathode.

Q. While charging the lead storage battery

$P b S O_{4}$ on anode is reduced to $P b$

$P b S O_{4}$ on cathode is reduced to $P b$

$P b S O_{4}$ on cathode is oxidized to $P b$

$P b S O_{4}$ on anode is oxidized to $P b O_{2}$

Q. While charging the lead storage battery

PbSO4​ on anode is reduced to Pb

PbSO4​ on cathode is reduced to Pb

PbSO4​ on cathode is oxidized to Pb

PbSO4​ on anode is oxidized to PbO2​

$P b S O_{4}$ on anode is reduced to $P b$

$P b S O_{4}$ on cathode is reduced to $P b$

$P b S O_{4}$ on cathode is oxidized to $P b$

$P b S O_{4}$ on anode is oxidized to $P b O_{2}$