Question

In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. Write the balanced chemical equation for the reaction. If 9.82 g SO2, react with excess oxygen and water, how many grams of H2SO4 are produced?

Answer 1

Answer:

The balanced reaction equation is:

2SO₂ + O₂ + 2H₂O $\rightarrow$ 2H₂SO₄

As you can see, the number of the moles of SO₂ reacted is equal to the number of the moles of H₂SO₄ produced:

$n(SO_2) = n(H_2SO_4)$

The molar mass $M$ of SO₂ is 64.06 g/mol. Let's calculate the number of the moles of SO₂:

$n(SO_2) = \frac{m}{M} = \frac{9.82}{64.06} = 0.153$ mol

The molar mass $M$ of H₂SO₄ is 98.08 g/mol. Then, the mass of H₂SO₄ produced is:

$m(H_2SO_4) = n·M = 0.153·98.08 =15.04$ g