Stoichiometry

Lead (II) sulfide, PbS, reacts with oxygen gas to produce lead (II) oxide, PbO, and sulfur dioxide, SO₂.

Groups:

(a) Reactants

,

(b) Products

Which is the balanced chemical equation for the following:  Lead(II) sulfide, PbS, reacts with oxygen gas to produce lead(II) oxide, PbO, and sulfur dioxide, SO₂?

• 2 times as much

• 2/3 as much

• 3/2 as much

• the same amount

Lead(II) sulfide, PbS, reacts with oxygen gas to produce lead(II) oxide, PbO, and sulfur dioxide, SO2. If 0.500 moles of O2 are used, then what would the B row contain?

• .333 for PbS, 0 for PbO, and 0 for SO₂

• .750 for PbS, 0 for PbO, and 0 for SO₂

• .333 for PbS, .333 for PbO, and .333 for SO₂

• .500 for PbS, 0 for PbO, and 0 for SO₂

Lead(II) sulfide, PbS, reacts with oxygen gas to produce lead(II) oxide, PbO, and sulfur dioxide, SO2. If 0.500 moles of O2 are used, then what would the C row contain?

• -.333 for PbS, +.333 for PbO, and +.333 for SO₂

• -.750 for PbS, +.750 for PbO, and +.750 for SO₂

• +.333 for PbS, -.333 for PbO, and -.333 for SO₂

• -.500 for PbS, +.500 for PbO, and +.500 for SO₂

Lead(II) sulfide, PbS, reacts with oxygen gas to produce lead(II) oxide, PbO, and sulfur dioxide, SO2. If 0.500 moles of O2 are used, then what would the A row contain?

• 0 for PbS, .333 for PbO, and .333 for SO₂

• 0 for PbS, .750 for PbO, and .750 for SO₂

• .333 for PbS, .333 for PbO, and .333 for SO₂

• 0 for PbS, .500 for PbO, and .500 for SO₂

How many grams are in .333 moles of PbO? (Molar Mass: 223.2 g/mol)

• .927

• 92.7%

• 93%

• 108%

Which is the limiting reactant?

• Oxygen gas will run out first, leaving .432 in excess CH₄

• Oxygen gas will run out first, leaving .863 in excess CH₄

• CH₄ will run out first, leaving .432 in excess O₂

• CH₄ will run out first, leaving .863 in excess O₂

What is the mass of CO₂ produced?

• 19.0 g of CO₂

• 18.990315 g of CO₂

• 38.0 g of CO₂

• 37.98063 g of CO₂