During the discharge of a lead storage battery, density of `H_(2)SO_(4)` fall from 1.3 to `1.14g//mL` Sulphuric acid of density `1.3g//ml` is 40W % and that of `1.14g//mL` is 20W% The battery holds two litre of the acid and volume remains practically constant during dicharging. The number of ampere- sec used from the battery is.

During the discharge of a lead storage battery, density of H_2SO_4 fell from 1.3 to 1.14 g/mL. Sulphuric acid of density 1.3g/ml is 40W% and that of 1.14g/mL is 20W%. The battery holds two litre of the acid and volume remains practically constant during discharging. The number of ampere-sec used from the battery is.

During the discharge of lead storage battery, the density of H_(2)SO_(4) fall from 1.3g/mL of 1.1g/mL. Sulphuric acid of density 1.3g/mL is 40% by weight and that of density 1.1g/mL is 20% by weight. The battery contains 2.0 litres of acid. The volume remains unchanged during discharge. How many faraday of current is liberated ?

During the discharge of lead storage battery, density of H_(2)SO_(4) fell from "1.294 to 1.139 g.cm"^(-3) . Sulphuric acid of density "1.294g.cm"^(-3) is 39% by mass and that of density "1.139 g.cm"^(-3) is 20% by mass. The battery holds 3.5L of acid and the volume remains practically constant during discharge. Calculate the no. of ampere-hours for which battery must have been used.

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) .

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139g // mL. Sulphuric acid of density 1.294 g // mL is 39% H_(2)SO_(4) by weight and that of density 1.139g // mL is 20% H_(2)SO_(4) by weight. The battery holds 3.5 L of the acid and the volume remained practically constant during the discharge. Calculate the number of ampere-hours for which the battery must have been used. The discharging reactions are Pb+ SO_(4)^(2-) rarr PbSO_(4) + 2e^(-) ( chargining) PbO_(2) + 4H^(+) + SO_(4)^(2-) + 2e^(-) rarr PbSO_(4) + 2H_(2) O ( dischargining)

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)