The percentage yield of the reaction between n-propanol and excess of acetic acid is 67.5%
How to determine the mass of n-propanol
- Volume = 0.59 mL
- Density = 0.803 g/mL
Mass = Density × Volume
Mass of n-propanol = 0.803 × 0.59
Mass of n-propanol = 0.47 g
Balanced equation
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Molar mass of n-propanol = 60.1 g/mol
Mass of n-propanol from the balanced = 1 × 60.1 = 60.1 g
Molar mass of propyl acetate = 102.1 g/mol
Mass of proply acetate from the balanced equation = 1 × 102.1 = 102.1 g
SUMMARY
From the balanced equation,
60.1 g of n-propanol reacted to produce 102.1 g of propyl acetate
How to determine the theoretical yield
From the balanced equation,
60.1 g of n-propanol reacted to produce 102.1 g of propyl acetate
Therefore,
0.47 g of n-propanol will react to produce = (0.47 × 102.1) / 60.1 = 0.8 g of propyl acetate
How to determine the percentage yield
- Actual yield of propyl acetate = 0.54 g
- Theoretical yield of propyl acetate = 0.8 g
Percentage yield = (Actual / Theoretical) × 100
Percentage yield = (0.54 / 0.8) × 100
Percentage yield = 67.5%
Learn more about stoichiometry:
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