One commercial system removes SO2 emission from 5 mole at 95∘C by the following set of reactions SO2(g)+Cl2(g)→SO2Cl2(g) SO2Cl2(g)+H2O(g)→H2SO4+HCl H2SO4+Ca(OH)2→CaSO4+H2OHow many gms of CaSO4 may be produced from 1.98gm of SO2

nSO2=1.9864=0.03 Mass of CaSO4=0.03×136=4.08

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One commercial system removes $S O_{2}$ emission from 5 mole at $95^{\circ} C$ by the following set of reactions
$S O_{2 (g)} + C l_{2 (g)} \to S O_{2} C l_{2 (g)}$
$S O_{2} C l_{2 (g)} + H_{2} O_{(g)} \to H_{2} S O_{4} + H C l$
$H_{2} S O_{4} + C a {(O H)}_{2} \to C a S O_{4} + H_{2} O$
How many gms of $C a S O_{4}$ may be produced from 1.98gm of $S O_{2}$

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answer is 4.

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Detailed Solution

$n S O_{2} = \frac{1.98}{64} = 0.03$

Mass of $C a S O_{4} = 0.03 \times 136 = 4.08$

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