During the discharge of a lead storage battery, the density of sulphuric acid fell from `1.294 g mL^(-1)` to `1.139 g mL^(-)`. Sulphuric acid of density `1.294 g mL^(-1)` is `39%` by weight and that of density `1.139 g mL^(-1)` is `20%` by weight. The battery hold `3.5` litre of acied and discharge. Calculate the no. of ampere hour for which the battery must have been used. The charging and discharging reactions are:
`Pb+SO_(4)^(2-) rarr PbSO_(4)+2e` (charging)
`PbO_(2)+4H^(+)+SO_(4)^(2-)+2e rarr PbSO_(4)+2H_(2)O` (discharging)

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294g mL^(-1) to 1.139g mL^(-1) . Sulphuric acid of dencity 1.294g mL^(-1) is 39% by weight and that of density 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 : Pb+SO_(4)^(2-)rarr PbSO_(4)+2e^(-) (charging) PbO_(2)+4H^(+)+SO_(4)^(2-)+2e^(-)rarr PbSO_(4)+2H_(2O) (dischargeing)

During discharge in the case of lead storage batteries density of sulphuric acid

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.13 to 1.15 g/ ml^(−1) and sulphuric acid of the density of 1.3 g/ ml^(−1) is 40% by mass and that of the density of 1.15 g/ ml^(−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: Pb+SO_(4)^(-2)rarrPbSO_(4)+2e^(-) (charging) PbO_(2)+4H^(+)+SO_(4)^(2-)+2erarrPnSO_(4)+2H_(2)O (discharging)

During the discharge of a lead storage battery, the density of sulphuric acid fell down from 1.294 to 1.139 g/ml. Sulphuric acid of density 1.294g/ml is 39% H_2SO_4 by weight and that of density of 1.139 g/ml is 20% H_2SO_4 by weight. The battery holds 3.5 L of acid and the volume remains practically constant during discharge. calculate the number of ampere hours for which the battery must have been used. The charging and discharging reactions are: Pb^(2+)+SO_4^(2-)LeftrightarrowPbSO_4+2bare(Charging) PbO_2+4H^(+)+SO_4^(2-)+2bareLeftrightarrowPbSO_4+2H2O(Discharging) .