Answer to Question #183987 in General Chemistry for Maddie

Question #183987

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)


1
Expert's answer
2021-04-23T07:30:02-0400

"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

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