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Standard XII
Chemistry
Question

Normalities of sulphuric acid before and after discharge are:
  1. 5.15,2.32
  2. 5.15,5.15
  3. 2.32,2.32
  4. 2.32,5.15

A
5.15,2.32
B
2.32,5.15
C
5.15,5.15
D
2.32,2.32
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Solution
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ANS; A
mass of sulfuric acid before discharge = 1.294 *3.5*1000*.39 = 1766.31 gm
normality of sulfuric acid before discharge = 1766.398×3.5
= 5.15 N
mass of sulfuric acid after discharge = 1.139 *3.5*1000*0.20 = 797.3 gm
normality of sulfuric acid after discharge = 797.398×3.5
= 2.32 N

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Normalities of sulphuric acid before and after discharge are:
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During discharge of a lead storage cell the density of sulphuric acid in the cell :
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Q4
During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139 g ml−1. Sulphuric acid of density 1.294g ml−1 is 39% by weight and that of density 1.139g ml−1 is 20% by weight. The battery holds 3.5 L of the acid and the volume remained practically constant during the discharge. Find the number of ampere-hours for which the battery must has been used.


The charging and discharging reactions are as follows:

Pb+SO2−4→PbSO4+2e− (charging)

PbO2+4H⊕+SO2−4+2e−→PbSO4+2H2O (discharging)

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Q5

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139 gmL−1. Sulphuric acid of density 1.294 gm L−1 is 39% by weight and that of density 1.139 gm L−1 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+SO42−→PbSO4+2e− (charging)

PbO2+4H++SO42−+2e−→PbSO4+2H2O (discharging)


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