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23 February, 18:21

1.16 g aspirin was synthesized from 1.03 g salicylic acid and 2.00 mL of acetic anhydride.

Calculate the mass percentage yield.

Molar mass of salicylic acid = 138.12 g/mol

Molar mass of aspirin = 180.16 g/mol

Density of acetic anhydride = 1.0820 g/mL

(Hint: It can be calculated by using actual / theoretical x100%)

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  1. 23 February, 18:50
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    The percentage yield is 85%

    Explanation:

    Step 1: The balanced equation

    2 C7H6O3 + (CH3CO) 2CO → 2 C9H8O4 + H20

    Step 2: Given data

    1.03 grams of salicylic acid

    2.00 mL of acetic anhydride.

    1.16 g aspirin was synthesized

    Step 3: Calculated moles of salicylic acid

    Number of moles of salicylic acid = mass of salicylic acid / Molar mass of salicylic acid

    Number of moles of salicylic acid = 1.03 grams / 138.12 g/mole

    Number of moles of salicylic acid = 0.0075 moles

    Step 4: Calculated moles of acetic anhydride

    Density = 1.0820 g/mL

    mass of acetic anhydride = 1.0820 * 2 mL = 2.164 grams

    Number of moles = 2.164 grams / 102.09 g/moles

    Number of moles = 0.0212 moles

    Step 5: find the limiting reactant

    C7H6O3 is the limiting reactant, there will react 0.0075 moles

    Since for 2 moles C7H6O3 consumed, we need 1 mole of (CH3CO) 2CO to produce 2 moles of C9H804

    So for 0.0075 moles C7H6O3 consumed, we produce 0.0075 moles of C9H8O4

    Step 6: Calculate mass of aspirin

    mass of aspirin = 0.0075 moles * 180 g/mole = 1.35 grams

    Step 7: Calculate the mass percentage yield

    (1.16 grams / 1.35 grams) * 100% = 85 %

    The percentage yield is 85%
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