What mass of carbon disulfide would have to be burned to produce a mixture of carbon disulfide and sulfur dioxide that masses 34.4 g?

Molar mass of CS₂ (carbon disulfide) = (12 + 32×2) g/mol = 76 g/mol
Molar mass of CO₂ (carbon dioxide) = (12 + 16×2) g/mol = 44 g/mol
Molar mass of SO₂ (sulfur dioxide) = (32 × 16 × 2) g/mol = 64 g/mol

Equation for the reaction :
CS₂ + 3O₂ → CO₂ + 2SO₂
OR: Mole ratio of CS₂ : CO₂ : SO₂ = 1 : 1 : 2

When 1 mole of CS₂ is burned, mass of the mixture of CO₂ and SO₂ produced
= (1 mol) × (44 g/mol) + (2 mol) × (64 g/mol)
= 172 g

When 34.4 g of a mixture of CO₂ and SO₂ is produced, the number of moles of CS₂ burned
= (34.4 g) / (172 g/mol)
= 0.2 mol

When 34.4 g of a mixture of CO₂ and SO₂ is produced, the mass of CS₂ burned
= (0.2 mol) × (76 g/mol)
= 15.2 g


====
Alternative method :

Mole ratio CS₂ : CO₂ : SO₂ = 1 : 1 : 2

Mass ratio CS₂ : (gas mixture formed) = 76 : (1×44 + 2×64) = 76 : 172

When 34.4 of the gas mixture is produced:
Mass ratio CS₂ : (gas mixture formed) = y : 34.4

y : 34.4 = 76 : 172
y = 34.4 × 76 / 172 = 15.2

Mass of CS₂ burned = 15.2 g