A) reduction of \[P{{b}^{2+}}\] to \[Pb\]
B) formation of \[PbS{{O}_{4}}\]
C) deposition of \[Pb\] at the anode
D) formation of \[Pb{{O}_{2}}\]
Correct Answer: A
Solution :
When a lead acid battery is charged, following reactions occur at anode and cathode. At anode: \[PbS{{O}_{4}}+2{{H}_{2}}O\xrightarrow{{}}Pb{{O}_{2}}+3{{H}^{+}}+HSO_{4}^{-}+2{{e}^{-}}\]At cathode: \[P{{b}^{2+}}+{{H}^{+}}+2{{e}^{-}}\xrightarrow{{}}Pb+HSO_{4}^{-}\] Thus, at cathode reduction of \[P{{b}^{2+}}\] to \[Pb\]occurs.
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