How many grams of carbon disulfide needed to completely consume 107L of chlorine gas according to the reaction at 25 °C and 1 atm?

Molar mass of CS₂ = (12.01 + 32.06×2) g/mol = 76.13 g/mol
(The molar mass you commonly use should be used instead.)

Consider the Cl₂ gas reacted :
Pressure, P = 1 atm
Volume, V = 107 L
Temperature, T = (273 + 25) K = 298 K
Gas constant, R = 0.08206 atm L / (mol K)

Gas law : PV = nRT
No. of moles of Cl₂, n = PV/(RT) = 1 × 107 / (0.08206 × 298) mol = 4.38 mol

CS₂ + 3Cl₂ → CCl₄ + S₂Cl₂
Mole ratio CS₂ : Cl₂ = 1 : 3
No. of moles of CS₂ needed = (4.38 mol) × (1/3) = 1.46 mol
Mass of CS₂ needed = (1.46 mol) × (76.13 g/mol) = 111 g

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