Lead (II) sulfide, PbS, reacts with oxygen gas to produce lead (II) oxide and dioxide. If 0.500 moles of O2 were consumed using this chemical reaction, how much of lead (II) would be produced?

Question

Lou

Chemistry

8 October, 19:20

Lead (II) sulfide, PbS, reacts with oxygen gas to produce lead (II) oxide and dioxide. If 0.500 moles of O2 were consumed using this chemical reaction, how much of lead (II) would be produced?

+5

Answers (1)

Know the Answer?

Baldie · Answer 1

I think you mean:

" ... reacts with oxygen gas to produce lead (II) oxide and 'sulfur' dioxide ... "

The balanced chemical reaction would be

2PbS + 3O2 - - > 2PbO + 2SO2

The stiochiometric ratio is this: 3 moles of O2 produces 2 moles of lead (II) oxide. So,

0.500 moles (2/3) = 0.333 moles

Therefore, 0.333 moles of PbO is produced when 0.500 moles of O2 reacts with PbS.