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10 April, 01:59

Calculate the theoretical yield of aspirin to be obtained when 2.0 g of salicylic acid and 5.0 mL of acetic anhydride (density = 1.08 g/mL) are mixed together. What is the limiting reagent?

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  1. 10 April, 02:28
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    The theoretical yield is 2.61 grams of aspirin

    salicylic acid is the limiting reactant.

    Explanation:

    Step 1: Data given

    Mass of salicylic acid = 2.0 grams

    Volume of acetic acid = 5.0 mL

    Density of acetic acid = 1.08 g/mL

    Molar mass of acetic anhydride = 102.09 g/mol

    Molar mass of salicylic acid = 138.12 g/mol

    Step 2: The balanced equation

    C7H6O3 + C4H6O3 → C9H8O4 + CH3COOH

    Step 3: Calculate mass of acetic acid

    Mass acid acid = density * volume

    Mass acetic acid = 1.08 g/mL * 5.0 mL

    Mass acetic acid = 5.5 grams

    Step 4: Calculate moles salicylic acid

    Moles salicylic acid = mass salicylic acid / molar mass salicylic acid

    Moles salicylic acid = 2.00 grams / 138.12 g/mol

    Moles salicylic acid = 0.0145 moles

    Step 5: Calculate moles acetic anhydride

    Moles acetic anhydride = 5.5 grams / 102.09 g/mol

    Moles acetic anhydride = 0.0538 moles

    Step 6: Calculate the limiting reactant

    For 1 mol salicylic acid we need 1 mol acetic anhydride to produce 1 mol aspirine.

    The limiting reactant is salicylic acid. It will completely be consumed. (0.0145 moles). Acetic anhydride will be in excess. There will react 0.0145 moles. There will remain 0.0538 - 0.0145 = 0.0393 moles

    Step 7: Calculate moles aspirine

    For 1 mol salicylic acid we need 1 mol acetic anhydride to produce 1 mol aspirine.

    For 0.0145 moles salicylic acid, we'll have 0.0145 moles aspirine

    Step 8: Calculate mass of aspirin

    Mass aspirin = moles aspirin * molar mass aspirin

    Mass aspirin = 0.0145 moles * 180.158 g/mol

    Mass aspirin = 2.61 grams = Theoretical yield

    The theoretical yield is 2.61 grams of aspirin

    salicylic acid is the limiting reactant.
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