During discharging of Pb storage battery, theconcentration of H2SO4 decrease with time. Calculatethe time, for which a current of 1 A can be drawnfrom the cell of 1 M initial concentration to 0.5 Mfinal concentration. (volume of solution5 lit).(assume volume remains same)

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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)

A lead storage battery containing 5.0L of $H_{2} S O_{4}$ solution is operated for $9.65 \times 10^{5} s$ with a steady current of 100 mA. Assuming volume of the solution remains constant, normality of $H_{2} S O_{4}$ will :

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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