Answer to Question #280869 in General Chemistry for Sib

Question

To obtain pure lead, lead (II) sulfide is burned in an atmosphere of pure oxygen. The products of the

reaction are lead and sulfur trioxide (SO3). Write a balanced chemical equation for this process. How many

grams of lead will be produced if 2.54 grams of PbS is burned with 1.88 g of O2? Express your answer to

the correct number of significant figures. Be sure to show all steps completed to arrive at the answer.

(Hint: be sure to work the problem with both PbS and O2)

Answer 1

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ: 239.27 32.00 207.2

2PbS + 3O₂ ⟶ 2Pb + 2SO₃

m/g: 2.54 1.88

2. Calculate the moles of each reactant

3. Calculate the moles of Pb from each reactant