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During the ch...

Question

During the charging of a lead storage battery the reaction at the cathode is-

A

P b \to P b^{2 +} + 2 e^{-}

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B

P b^{2 +} + 2 e^{-} \to P b

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C

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

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D

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

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Solution

The correct option is B $P b^{2 +} + 2 e^{-} \to P b$
Reduction takes place at cathode

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Similar questions

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

H_{2} S O_{4}

1.294

1.139

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

i s

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

i s

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

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. During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139

g m L^{- 1}

H_{2} S O_{4}

1.294 g m L^{- 1}

is 39% and that of density

1.139 g m L^{- 1}

is 20% by weight.The battery holds 3.5 L of acid and the volume practically remains constant during discharge. The number of ampere hours for which the battery must have been used are........................
The discharging and charging reactions are:

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

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

During the discharge of a lead storage battery, the density of sulphuric acid fell from $1.294$ to $1.139$ gm $L^{- 1}$ . Sulphuric acid of density $1.294$ gm $L^{- 1}$ is $39$ % by weight and that of density 1.139 gm $L^{- 1}$ is $20$ % by weight. The battery holds $3.5$ litres of acid and the column practically remained constant during the discharge.

Calculate the number of ampere-hours for which the battery must have been used. The charging and discharging reactions are :

$P b + S O {_{4}}^{2 -} \to P b S O_{4} + 2 e^{-}$ (charging)

$P b O_{2} + 4 H^{+} + S O {_{4}}^{2 -} + 2 e^{-} \to P b S O_{4} + 2 H_{2} O$ (discharging)

Q. During the discharge of a lead storage battery, the density of sulphuric acid fell from

1.294

1.139 g m l^{- 1}

. Sulphuric acid of density

1.294 g m l^{- 1}

is 39% by weight and that of density

1.139 g m l^{- 1}

is 20% by weight. The battery holds 3.5 L of the acid and the volume remained practically constant during the discharge. Find the number of ampere-hours for which the battery must has been used.

The charging and discharging reactions are as follows:

$P b + S O_{4}^{2 -} \to P b S O_{4} + 2 e^{-}$ (charging)

$P b O_{2} + 4 H^{\oplus} + S O_{4}^{2 -} + 2 e^{-} \to P b S O_{4} + 2 H_{2} O$ (discharging)

Q. During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139 g

m l^{- 1}

and sulphuric acid of the density of 1.294 g

m l^{- 1}

is 39% by mass and that of the density of 1.139 g

m l^{- 1}

is 20% by mass. The battery holds 3.5 litre of acid and the volume practically remained constant during the discharge. Calculate the no. of ampere hour for which the battery must have been used. The charging and discharging reactions are:

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

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

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