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Question

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139 gmL1. Sulphuric acid of density 1.294 gm L1 is 39% by weight and that of density 1.139 gm L1 is 20% by weight. The battery holds 3.5 litres of acid and the column practically remained constant during the discharge.

Calculate the number of ampere-hours for which the battery must have been used. The charging and discharging reactions are :

Pb+SO42PbSO4+2e (charging)

PbO2+4H++SO42+2ePbSO4+2H2O (discharging)


A
297
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B
189
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C
274
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D
200
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Solution

The correct option is A 297
Mass of sulphuric acid consumed:
1.294g1mL×3500mL=4529g

1.139g1mL×3500mL=3986g

weight consumed=4529-3986=543 g
moles of sulphuric acid =54398=5.54moles
moles of electrons consumed = 11 moles
total charge =96500×11=1069377 C
=10693773600=297 A-hr

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