Sulfur dioxide gas reacts with oxygen gas and water according to the chemical reaction below. When 4.5 g of SO₂ are mixed with excess O₂ and H₂O, how many grams of H₂SO₄ are produced
2SO₂(g) + O₂(g) + 2H₂O(l) $\rarr$ 2H₂SO₄(l)

Question

Sulfur dioxide gas reacts with oxygen gas and water according to the chemical reaction below. When 4.5 g of SO₂ are mixed with excess O₂ and H₂O, how many grams of H₂SO₄ are produced
2SO₂(g) + O₂(g) + 2H₂O(l)

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2H₂SO₄(l)

Quizplus · Accepted Answer

First, we need to correct the chemical equation and interpret it correctly: $2 SO_2 (g) + O_2 (g) + 2 H_2O (l) \rightarrow 2 H_2SO_4 (l)$. The molar mass of $SO_2$ is approximately 64 g/mol. Given 4.5 g of $SO_2$, we have $\frac{4.5}{64}$ moles of $SO_2$, which is roughly 0.0703 moles. The stoichiometry of the reaction shows that the moles of $H_2SO_4$ produced will be the same as the moles of $SO_2$ reacted, assuming $SO_2$ is the limiting reactant. The molar mass of $H_2SO_4$ is approximately 98 g/mol. Therefore, the mass of $H_2SO_4$ produced is $0.0703 \times 98 \approx 6.9$ g.

Sulfur Dioxide Gas Reacts with Oxygen Gas and Water According →\rarr→

Sulfur Dioxide Gas Reacts with Oxygen Gas and Water According $\rarr$