One commercial system removes SO₂ emissions from smoke at 95.0°C by the following set of balanced reactions:
SO₂ + Cl₂ $\to$ SO₂Cl₂
SO₂Cl₂ + 2H₂O $\to$ H₂SO₄ + 2HCl
H₂SO₄ + Ca(OH) ₂ $\to$ CaSO₄ + 2H₂O
Assuming the process is 95.0% efficient,how many grams of CaSO₄ may be produced from 100.grams of SO₂?
(molar masses: SO₂,64.1 g/mol;CaSO₄,136 g/mol)

Question

One commercial system removes SO₂ emissions from smoke at 95.0°C by the following set of balanced reactions:
SO₂ + Cl₂

\to

SO₂Cl₂
SO₂Cl₂ + 2H₂O

\to

H₂SO₄ + 2HCl
H₂SO₄ + Ca(OH) ₂

\to

CaSO₄ + 2H₂O
Assuming the process is 95.0% efficient,how many grams of CaSO₄ may be produced from 100.grams of SO₂?
(molar masses: SO₂,64.1 g/mol;CaSO₄,136 g/mol)

Quizplus · Accepted Answer

The Answer of One commercial system removes SO₂ emissions from smoke at 95.0°C by the following set of balanced reactions: SO₂ + Cl₂ $\to$ SO₂Cl₂ SO₂Cl₂ + 2H₂O $\to$ H₂SO₄ + 2HCl H₂SO₄ + Ca(OH)₂ $\to$ CaSO₄ + 2H₂O Assuming the process is 95.0% efficient,how many grams of CaSO₄ may be produced from 100.grams of SO₂? (molar masses: SO₂,64.1 g/mol;CaSO₄,136 g/mol)

One Commercial System Removes SO2 Emissions from Smoke at 95 →\to→

One Commercial System Removes SO₂ Emissions from Smoke at 95 $\to$