The mass of SO₃ produced is 954 g
How to determine the theoretical yield
C₄H₈S₂ + 9O₂ —> 4CO₂ + 4H₂O + 2SO₃
Molar mass of C₄H₈S₂ = (12×4) + (8×1) + (32×2) = 120 g/mol
Mass of C₄H₈S₂ from the balanced equation = 1 × 120 = 120 g
Molar mass of SO₃ = 32 + (16×3) = 80 g/mol
Mass of SO₃ from the balanced equation = 2 × 80 = 160 g
SUMMARY
From the balanced equation above,
120 g of C₄H₈S₂ reacted to produce 160 g of SO₃.
Therefore,
750 g of C₄H₈S₂ will react to produce = (750 × 160)/120 = 1000 g of SO₃
Thus, the theoretical yield SO₃ is 1000 g
How to determine the actual yield
- Percentage yield = 95.4%
- Theoretical yield = 1000 g
Actual yield = percent × theoretical
Actual yield = 95.4% × 1000
Actual yield = 954 g
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