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Q.

4 g of sulphur is burnt to form SO₂, which is oxidised by Cl₂ water. The solution is then treated with BaCl₂ solution.
The amount of BaSO₄ precipitated is:

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a

0.24 mol

b

0.5 mol

c

1 mol

d

0.125 mol

answer is D.

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Detailed Solution

Moles of S = $\frac{4}{32} = \frac{1}{8} = 0.125 mol$

S+O₂ $\overset{}{\to}$ SO₂

SO₂+Cl₂ $\overset{}{\to}$ $2 {Cl}^{⊝} + {SO}_{4}^{2 -}$

${SO}_{4}^{2 -} + {BaCl}_{2} \overset{}{\to {BaSO}_{4} + 2 {Cl}^{⊝}}$

Moles of S = Moles of SO₂ = Moles of ${SO}_{4}^{2 -}$

= Moles of BaSO₄ = 0.125 mol

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