please answer this chemistry problem

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

This equation seems balanced from the get-go. The moles of Cu, S, and O match on both sides of the equation. If 1233 g of Cu are being produced, and we know that 1 mole of Cu is proportional to 1 mole of SO₂, then we can convert grams of Cu to moles of Cu and therefore we have moles of SO₂. From there we just need to convert moles of SO₂ into grams to get the mass of gaseous SO₂ that will be produced.

1233 g Cu(s) * 1mole Cu (s)/63.55g = 19.40 moles of Cu(s)

19.4 moles of Cu(s) * 1mole SO₂ (g)/1mole Cu(s) * 64g/1mole SO₂ (g) = 1241.7 g of SO₂ (g) produced