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Secondary Cells

During discha...

Question

During discharging of a lead storage battery, which of the following is/are true?

H_{2} S O_{4}

is produced

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H_{2} O

is consumed

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P b S O_{4}

is formed at both electrodes

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Density of electrolytic solution decreases

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Solution

The correct options are
C Density of electrolytic solution decreases
D $P b S O_{4}$ is formed at both electrodes
Oxidation at anode is represented by the half cell reaction:
$P b (s) + S O_{4}^{2 -} (a q) \to P b S O_{4} (s) + 2 e^{-}$
Reduction at cathode is represented by the half cell reaction:
$P b O_{2} (s) + 4 H^{+} (a q) + S O_{4}^{2 -} (a q) + 2 e^{-} \to P b S O_{4} (s) + 2 H_{2} O (l)$
The overall cell reaction is:
$P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} (a q) \to 2 P b S O_{4} (s) + 2 H_{2} O (l)$ .
During discharging of a lead storage battery, sulfuric acid is consumed and water is produced.
Lead sulphate is formed at both electrodes.
Since sulfuric acid is consumed, the density of the electrolytic solution decreases.

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Similar questions

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 :

(c h a r g i n g)

g m L^{- 1}

H_{2} S O_{4}

1.294 g m L^{- 1}

1.139 g m L^{- 1}

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

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

H_{2} 3 O_{4}

When a lead storage battery is discharged, which of the following is true?

During discharging of lead-storage acid battery following reaction takes place:

P b (s) + P b O_{2} (s) + 2 H_{2} S O_{4} \to 2 P b S O_{4} (s) + 2 H_{2} O

If 2.5 amp of current is drawn for 965 minutes, $H_{2} S O_{4}$ consumed is:

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