Question

What mass (in grams) of aspirin (C₉H₈O₄) is produced from 57.6 g of C₇H₆O₃ assuming 95.0% yield from the reaction below? C₇H₆O₃ (s) + C₄H₆O₃ (s) → C₉H₈O₄ (s) + HC₂H₃O₂ (aq).

Answer 1

Answer:

78.15 g

Explanation:

Number of moles of C₇H₆O₃ that reacted = mass/molar mass = 57.6g/126 gmol-1

Number of moles of C₇H₆O₃ = 0.457 moles of C₇H₆O₃

From the reaction equation;

1 mole of C₇H₆O₃ yields one mole of aspirin

0.457 moles of C₇H₆O₃ yields C₇H₆O₃ of aspirin

Hence theoretical yield of aspirin = 0.457 moles × 180 gmol-1 = 82.26g of aspirin

% yield = actual yield/theoretical yield ×100

Actual yield= % yield × theoretical yield/100

Actual yield = 95.0 × 82.26/100

Actual yield = 78.15 g