The minimum quantity of benzene, C₆H₆ needed for the reaction is 106.67 g
<h3>How to determine the theoretical yield of chlorobenzene, C₆H₅Cl</h3>
From the question given, the following data were obtained
- Actual yield = 100 g
- Percentage yield = 65%
- Theoretical yield =?
Percentage yield = (Actual / Theoretical) × 100
65% = 100 / Theoretical
0.65 = Actual / Theoretical
Cross multiply
0.65 × Theoretical = 100
Divide both sides by 0.65
Theoretical = 100 / 0.65
Theoretical yield = 153.85 g
<h3>How to determine the mass of benzene, C₆H₆ needed</h3>
Balanced equation
C₆H₆ + Cl₂ → C₆H₅Cl + HCl
Molar mass of C₆H₆ = 78 g/mol
Mass of C₆H₆ from the balanced equation = 1 × 78 = 78 g
Molar mass of C₆H₅Cl = 112.5 g
Mass of C₆H₅Cl from the balanced equation = 1 × 112.5 = 112.5 g
SUMMARY
From the balanced equation above,
112.5 g of C₆H₅Cl were obtained from 78 g of C₆H₆
Therefore,
153.85 g of C₆H₅Cl will be produced from = (153.85 × 78) / 112.5 = 106.67 g of C₆H₆
Thus, the minimum amount of benzene, C₆H₆ needed for the reaction is 106.67 g
Learn more about stoichiometry:
brainly.com/question/16735180
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