Answer to Question #183987 in General Chemistry for Maddie

Question

Calculate the mass of gaseous SO₂ that will be produced along with 1233 g of copper from the roasting of copper(II) sulfide.

CuS(s) + O₂(g)  Cu(s) + SO₂(g)

Answer 1

$CuS_{(s) }+ O_{2(g)} \to Cu_{(s)} + SO_{2(g)}$

molar mass of copper = 65.5g

number of moles of copper = 1233/65.5 = 18.8 moles

1 mole of copper is produced by 1 mole of SO₂

1 mole of CuS produces 1 mole of SO₂

1 moles of CuS produces 64.06g of SO₂

$\therefore$ 18.8 moles of CuS produces 1204.32g of SO₂