The percent yield of CCl₄ from the reaction of 18.0 g of carbon disulphide with 22.0 grams of Cl₂ is 77.3%
Equation of reaction:
CS₂ + 3 Cl₂ ----> CCl₄ + S₂Cl₂
molar mass of CS₂ = 78 g/mol
molar mass of Cl₂ = 71 g/mol
molar mass of CCl₄ = 154 g/mol
- 1 mole of carbon disulphide reacts with 3 moles of chlorine gas
78 g of CS₂ reacts with * 71 g of Cl₂
78 g of CS₂ reacts with 213 g of Cl₂
18 g of CS₂ reacts with 213 * 18/ 78 g of Cl₂
18 g of CS₂ requires 49.1 g of Cl₂
- Therefore, Cl₂ is the limiting reactant
3 moles of Cl₂ produces 1 mole of CCl₄
213 g of Cl₂ produces 154 g of CCl₄
22.0 g of Cl₂ will produce 154 * 22 / 213 g of CCl₄
22.0 g of Cl₂ will produce 15.9 g of CCl₄
- Percent yield = (actual yield / expected yield) * 100%
Actual yield = 12.3 g
Expected yield = 15.9 g
Percent yield = 12.3/15.9) * 100%
Percent yield = 77.3 %
The percent yield of CCl₄ from the reaction of 18.0 g of carbon disulphide with 22.0 grams of Cl₂ is 77.3%
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