The roasting of Cu₂S(s)produces Cu(s)and SO₂(g).What mass of sulfur dioxide is produced by the roasting of 1.00 × 10³ kg Cu₂S(s)? Cu₂S(s)+ O₂(g)→ 2Cu(s)+ SO₂(g)

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Quizplus · Accepted Answer

The balanced chemical equation shows that 1 mole of Cu2S produces 1 mole of SO2. The molar mass of Cu2S (Cu = 63.55, S = 32.07, Cu2S = 2*63.55 + 32.07 = 159.17 g/mol) and SO2 (S = 32.07, O = 16.00, SO2 = 32.07 + 2*16.00 = 64.07 g/mol) are used for conversion. Given 1.00 × 10^3 kg (or 1,000,000 g) of Cu2S, the mass of SO2 produced can be calculated using stoichiometry. The calculation follows the ratio derived from the molar masses and the balanced equation, leading to approximately 402 kg of SO2 produced.

The Roasting of Cu2S(s)produces Cu(s)and SO2(g)

The Roasting of Cu₂S(s)produces Cu(s)and SO₂(g)