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

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2/3 as much

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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, what would the B row contain?

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

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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, what would the C row contain?

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

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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, what would the A row contain? Options: 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.

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

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

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92.7%

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Which is the limiting reactant? Options: 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

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

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What is the mass of CO₂ produced?

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19.0 g of CO₂