Answer:
SO₂ + 0.5 O₂ + H₂O → H₂SO₄
3.83 g
Explanation:
In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. The balanced chemical equation is:
SO₂ + 0.5 O₂ + H₂O → H₂SO₄
The molar mass of SO₂ is 64.07 g/mol. The moles of SO₂ corresponding to 2.50 g are:
2.50 g × (1 mol/64.07 g) = 0.0390 mol
The molar ratio of SO₂ to H₂SO₄ is 1:1. The moles of H₂SO₄ formed are 0.0390 moles.
The molar mass of H₂SO₄ is 98.08 g/mol. The mass of H₂SO₄ is:
0.0390 mol × 98.08 g/mol = 3.83 g
The mass of acid rain produced by the reaction of 2.50 of sulfur dioxide with oxygen has been 3.83 grams.
The balanced chemical equation can be defined as the chemical equation in which the reactants and products have been equal.
The balanced chemical equation for acid rain has been:
[tex]\rm SO_2\;+\;\dfrac{1}{2}\;O_2\;+\;H_2O\;\rightarrow\; H_2SO_4[/tex]
Thus, from the equation, 1 mole of sulfur dioxide has resulted in the formation of 1 mole of sulfuric acid.
The moles of sulfur dioxide has been given as:
Moles = [tex]\rm \dfrac{weight}{molecular\;weight}[/tex]
Moles of sulfur dioxide = [tex]\rm \dfrac{2.50}{64.07}[/tex]
Moles of sulfur dioxide = 0.0390 mol.
Since 1 mole sulfur dioxide = 1 mole sulfuric acid
0.0390 mol sulfur dioxide = 0.0390 mol Sulfuric acid
The mass of sulfuric acid = Moles × Molecular mass
Mass of 0.0390 mol sulfuric acid = 0.0390 mol × 98.08 g/mol
Mass of sulfuric acid = 3.83 grams.
Thus, the mass of acid rain produced by the reaction of 2.50 of sulfur dioxide with oxygen has been 3.83 grams.
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