One commercial system removes SO2 emission from smoke at 95 - C by the following set of reaction- SO2g-Cl2g - SO2Cl2g SO2Cl2g-H2Ol - H2SO4-HCl H2SO4-CaOH2- CaSO4-H2OGrams of CaSO4 that may be produced from 3-78 g of SO2 are -

The reactions are as follows: SO_2(g)+Cl_2(g) → SO_2Cl_2(g) SO_2Cl_2(g)+H_2O(l) → H_2SO_4+HCl H_2SO_4+Ca(OH)_2→ CaSO_4+H_2O From reactions, we can ...

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Standard XII

Chemistry

Stoichiometric Calculations

One commercia...

Question

One commercial system removes $S O_{2}$ emission from smoke at $95^{\circ} C$ by the following set of reaction:
$S O_{2} (g) + C l_{2} (g) \to S O_{2} C l_{2} (g)$
$S O_{2} C l_{2} (g) + H_{2} O (l) \to H_{2} S O_{4} + H C l$
$H_{2} S O_{4} + C a (O H)_{2} \to C a S O_{4} + H_{2} O$
Grams of $C a S O_{4}$ that may be produced from $3.78 g$ of $S O_{2}$ are :

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Solution

The reactions are as follows:
$S O_{2} (g) + C l_{2} (g) \to S O_{2} C l_{2} (g)$
$S O_{2} C l_{2} (g) + H_{2} O (l) \to H_{2} S O_{4} + H C l$
$H_{2} S O_{4} + C a (O H)_{2} \to C a S O_{4} + H_{2} O$
From reactions, we can see that one mole of $S O_{2}$ produces one mole of $C a S O_{4}$ .
Moles of $S O_{2}$ (given) $= \frac{3.78}{64} = 0.0590$ mol.
So, mass of $C a S O_{4}$ produced $= 0.0590 \times 136 = 8$ g.

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Similar questions

Q. A commercial system removes

S O_{2}

emission from smoke at

95^{\circ} C

by the following set of reactions:

S O_{2} + C l_{2} \to S O_{2} C l_{2} (Yield = 75 %)

S O_{2} C l_{2} + 2 H_{2} O \to H_{2} S O_{4} + 2 H C l (Yield = 80 %)

H_{2} S O_{4} + C a (O H)_{2} \to C a S O_{4} + 2 H_{2} O (Yield = 100 %)

How many grams of

C a S O_{4}

may be produced from 3.78 g of

S O_{2}

Q. A commercial system removes

S O_{2}

emission from smoke at

95^{\circ} C

by the following set of reactions:

S O_{2} + C l_{2} \to S O_{2} C l_{2} (Yield = 75 %)

S O_{2} C l_{2} + 2 H_{2} O \to H_{2} S O_{4} + 2 H C l (Yield = 80 %)

H_{2} S O_{4} + C a (O H)_{2} \to C a S O_{4} + 2 H_{2} O (Yield = 100 %)

How many grams of

C a S O_{4}

may be produced from 3.78 g of

S O_{2}

Q. Which of the following chemical reactions depicts the oxidising behaviour of

H_{2} S O_{4}

Which of the following chemical reaction depicts the oxidizing behavior of $H_{2} S O_{4}$ ?

Q. On heating a mixture of

S O_{2} C l_{2}

, and CO two equilibria are simultaneously established :-

S O_{2} C l_{2} (g) ⇌ S O_{2} (g) + C l_{2} (g)

C O (g) + C l_{2} (g) ⇌ C O C l_{2} (g)

on adding more

S O_{2}

at equilibrium what will happen?

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One commercial system removes SO2 emission from smoke at 95∘C by the following set of reaction:SO2(g)+Cl2(g)→SO2Cl2(g)SO2Cl2(g)+H2O(l)→H2SO4+HClH2SO4+Ca(OH)2→CaSO4+H2OGrams of CaSO4 that may be produced from 3.78g of SO2 are :

The reactions are as follows:SO2(g)+Cl2(g)→SO2Cl2(g)SO2Cl2(g)+H2O(l)→H2SO4+HClH2SO4+Ca(OH)2→CaSO4+H2OFrom reactions, we can see that one mole of SO2 produces one mole of CaSO4.Moles of SO2 (given) =3.7864=0.0590 mol.So, mass of CaSO4 produced =0.0590×136=8 g.