A lead storage cell is discharged which causes the H₂SO₄ electrolyte to change from a concentration of 40% by weight (density = 1.260 g/ml) to 28%, by weight. The original volume of solution was 1L. Identify the correct statement(s);

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The overall cell reaction is:

$Pb (s) + {PbO}_{2} (s) + 2 H_{2} {SO}_{4} (aq) \to 2 {PbSO}_{4} (s) + 2 H_{2} O (ℓ)$

A total of 2.0 moles of H₂SO₄ is reacted

The total charge released from anode of the cell is 1.93 x 10⁵ coulomb

The mass of electrolytic solution has decreased

answer is A, B, C, D.

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Detailed Solution

Net cell reaction of discharge is
$Pb + {PbO}_{2} + \underset{x mole}{2 H_{2} {SO}_{4}} \to 2 {PbSO}_{4} + \underset{x mole}{2 H_{2} O}$
Initial mass of H₂SO₄ , $W_{1} = 10 \times 1.26 \times \frac{40}{100} = 504 gm$
Final mass of H₂SO₄, $W_{2} = (1260 - 98 x + 18 x) \times \frac{28}{100} = (352.8 - 22.4 x) gm$
From reaction, 504 - 98x = 352.8 - 22.4x $\Rightarrow$ x = 2