During the discharge of a lead storage battery, the density of `40% H_(2)SO_(4)` by weight fell from `1.225 ` to `0.98 (` which is `20%` by weight `).` What is the change in molarities of `H_(2)SO_(4)`?

During the discharge of a lead storage battery, the density of 40% H_(2)SO_(4) by weight fell from 1.225 to 0.98 (which is 20% by weight). What is the charge in molarities of H_(2)SO_(4) ?

During the discharge of a lead storage battery the density of H_(2)SO_(4) talls from rho_(1)g//cc to rho_(2)g//C , H_(2)SO_(4) of density of rho_(1)g//C . C is X% by weight and tat of density fo rho_(2)gc.c is Y% by weight. The battery holds V litre of acid before discharging. Calculate the total charge released at anode of the battery. The reactions occurring during discharging are ltbr. At anode: Pb+SO_(4)^(2-)toPbSO_(4)+2e^(-) At cathode: PbO_(2)+4H^(+)+SO_(4)^(2-)+2e^(-)toPbSO_(4)+2H_(2)O

During the discharge of a lead storage battery the density of H_(2)SO_(4) talls from rho_(1)g//cc to rho_(2)g//C , H_(2)SO_(4) of density of rho_(1)g//C . C is X% by weight and tat of density fo rho_(2)gc.c is Y% by weight. The battery holds V litre of acid before discharging. Calculate te total charge released at anode of the battery. The reactions occurring during discharging are ltbr. At anode: Pb+SO_(4)^(2-)toPbSO_(4)+2e^(-) At cathode: PbO_(2)+4H^(+)+SO_(4)^(2-)+2e^(-)toPbSO_(4)+2H_(2)O

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 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 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.