During discharging of lead-storage acid battery following reaction takes place- Pbs-PbO2s-2H2SO4- 2PbSO4s-2H2OIf 2-5 amp of current is drawn for 965 minutes- H2SO4 consumed is-

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Standard XII

Chemistry

Secondary Cells

During discha...

Question

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:

0.75 mol

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3.00 mol

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1.50 mol

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4.50 mol

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Solution

The correct option is C 3.00 mol
The moles of sulfuric acid can be calculated by using the expression.
Moles of acid consumed = Moles of electrons passed x mole ratio
Substitute values in the above expression.
Moles of acid consumed $= \frac{2.5 A \times 57900 s}{96500} m o l e^{-} \times \frac{2 m o l a c i d}{1 m o l l e a d} = 3$ mol.

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Similar questions

Q. When lead-acid accumulator (battery) is discharged, the following reaction takes place.

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

1.25 A

average current is drawn for a period of 1930 minutes, the mass of

H_{2} S O_{4}

consumed is :

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. A lead storage cell is discharged which causes the

H_{2} S O_{4}

electrolyte from a concentration of

34.6

% by mass (density 1.261 g

m l^{- 1}

28^{o} C

) to one of

27

% by mass. The original volume of electrolyte is one litre. How many Faraday have left the anode of battery? Note the water is produced by the cell reaction and

H_{2} S O_{4}

is used up. Overall reaction is :

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

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}

of density

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^{-}

(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)

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During discharging of lead-storage acid battery following reaction takes place:Pb(s)+PbO2(s)+2H2SO4→2PbSO4(s)+2H2OIf 2.5 amp of current is drawn for 965 minutes, H2SO4 consumed is:

The correct option is C 3.00 molThe moles of sulfuric acid can be calculated by using the expression. Moles of acid consumed = Moles of electrons passed x mole ratioSubstitute values in the above expression.Moles of acid consumed =2.5A×57900s96500mole−×2 mol acid1 mol lead=3 mol.

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: