The reaction for the burning of one type of match tip is as follows: P4S3(s) + 8O2(g) △→ P4O10(g) + 3SO2(g) What volume of SO2 at STP can be produced by burning 1.00 grams of P4S3 in excess O2?

Answer 1

P₄S₃(s) + 8O₂(g) △→ P₄O₁₀(g) + 3SO₂(g) ... balanced equation

Using dimensional analysis to find moles of SO2 produced, we have...

1.00 g P₄S₃ x 1 mol P₄S₃ / 221 g x 3 mol SO₂ / 1 mol P₄S₃ = 0.01357 moles SO₂

Now, since the reaction takes place at STP, we know that 1 mole of any ideal gas = 22.4 L.

Thus,...

0.01357 moles SO2 x 22.4 L/mol = 0.304 liters (to 3 significant figures)