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Standard XII

Chemistry

Electrolytic Cell

While chargin...

Question

While charging the lead storage battery, ………

PbSO₄on anode is reduced to Pb

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PbSO₄ on cathode is reduced to Pb

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PbSO₄on cathode is oxidized to Pb

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PbSO₄ on anode is oxidized to PbO₂

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Solution

The correct option is D i.e PbSO₄on the anode is reduced to Pb
A lead Storage battery is a secondary cell.
In a lead storage battery, Anode is the negative electrode that lose electrons to the external circuit and oxidizes during an electrochemical reaction while the cathode is the positive electrode that gains electrons from the external circuit and is reduced during the electrochemical reaction.

Anode: Pb will convert into $P b S O_{4}$
Cathode: PbO $_{2}$ will convert into $P b S O_{4}$
When charging is done for a lead storage battery, the reaction will reverse, so $P b S O_{4}$ will convert into Pb on the anode. On cathode, $P b S O_{4}$ will convert into $P b O_{2}$

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Similar questions

Electrochemical Battery

An electrochemical battery is a device powered by oxidation and reduction reactions that are physically separated. So that the electrons must travel through a wire from the reducing agent to the oxidizing agent.

The reducing agent loses electrons and is oxidized in a reaction that takes place at an electrode is called the anode. The oxidizing agent gains electrons and is reduced in a reaction that takes at an electrode is called the cathode.

To maintain a net zero charge in each compartment, there is a limited flow of ions through a salt bridge.

For example, in a car battery the reducing agent is oxidized by the following reaction, which involves a lead (

P b

) anode and sulfuric acid (

H_{2} S O_{4}

). Lead sulfate (

P b S O_{4}

), protons (

H

), and electrons (

e^{-}

) are produced.

At the cathode, the below reaction occurs :

P b O_{2} + H_{2} S O_{4} + 2 H^{+} + 2 e^{-} \to

PbSO_4+2H_2O$

At the anode, the below reaction occurs :

P b + H_{2} S O_{4} \to P b S O_{4} + 2 H^{+} + 2 e^{-}

Electrons are produced by a chemical reaction that takes place at the:

Q. In a lead storage battery, the anode reaction is,

P b + H_{2} S O_{4} \to P b S O_{4} + 2 H^{+} + 2 e^{-}

Weight in g of Pb would be used up for battery to use for 1 ampere hour is___________. (write the nearest integer value)

Q. During the discharge of a lead storage battery, density of

H_{2} S O_{4}

fell from

1.294

1.139

\ g/mL

. S u l p h u r i c a c i d o f d e n s i t y

1.294

i s

H_{2}SO_{4}

b y w e i g h t a n d t h a t o f d e n s i t y

1.139\ g/mL

i s

H_{2}SO_{4}

b y w e i g h t . T h e b a t t e r y h o l d

3.5\ litre

o f t h e a c i d a n d v o l u m e r e m a i n s p r a c t i c a l l y c o n s t a n t d u r i n g d i s c h a r g e . C a l c u l a t e a m p e r e - h o u r o f w h i c h t h e b a t t e r y m u s t h a v e b e e n u s e d . T h e c h a r g i n g a n d d i s c h a r g i n g r e a c t i o n s a r e :

Pb + SO_{4}^{2-} \rightarrow PbSO_{4} + 2e^{-}

(c h a r g i n g)

PbO_{2} + 4H^{+} + SO_{4}^{2-} + 2e^{-}\rightarrow PbSO_{4} + 2H_{2}O$ (discharging).

Q. The electrode reactions for charging of a lead battery are:

P b S O_{4} + 2 e \to P b + S O_{4}^{2 -}

P b S O_{4} + 2 H_{2} O \to P b O_{2} + S O_{4}^{2 -} + 4 H + 2 e

The electrolyte in the battery is an aqueous solution of

H_{2} 3 O_{4}

. After this battery has been charged:

Q. Conversion of

P b S O_{4}

P b S

is :

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