Ask Question
8 June, 18:36

Suppose that in the synthesis of isoamyl acetate by Fisher esterification, a student began with 6.103 grams of acetic acid and 3.728 grams of isoamyl alcohol. If the mass of isoamyl acetate obtained were 4.993, what was the percent yield? (If your answer is not quite the same as one of the answers below, then choose the closest value.)

+3
Answers (1)
  1. 8 June, 22:12
    0
    The % yield is 90.68 %

    Explanation:

    Step 1: Data given

    Mass of acetic acid = 6.103 grams

    Mass of isoamyl alcohol = 3.728 grams

    Mass isoamyl acetate obtained = 4.993 grams

    Molar mass acetic acid = 60.05 g/mol

    Molar mass of isoamyl alcohol = 88.15 g/mol

    Molar mass of isoamyl acetate = 130.19 g/mol

    Step 2: The balanced equation

    C5H12O + CH3COOH → C7H14O2 + H2O Isoamyl alcohol + acetic acid - --> Isoamyl acetate + water

    Step 3: Calculate moles of acetic acid

    Moles acetic acid = Mass acetic acid / Molar mass acetic acid

    Moles acetic acid = 6.103 grams / 60.05 g/mol

    Moles acetic acid = 0.1016 moles

    Step 4: Calculate moles isoamyl alcohol

    Moles isoamyl alcohol = 3.728 grams / 88.15 g/mol

    Moles isoamy lalcohol = 0.04229 moles

    Step 5: Calculate limiting reactant

    The mole ratio is 1:1 so isoamyl alcohol has the smallest number of moles. So isoamyl alcohol is the limiting reactant. It will be completely be consumed (0.04229 moles).

    Acetic acid is in excess, there will be consumed 0.04229 moles.

    There will remain 0.1016 - 0.04229 = 0.05931‬ moles

    Step 6: Calculate moles of isoamyl acetate

    For 1 mole acetic acid, we need 1 mole of isoamyl alcohol, to produce 1 mole isoamyl acetate and 1 mole of H2O

    For 0.04229 moles isoamyl alcohol consumed, there will be produced 0.04229 moles of isoamyl acetate.

    Step 7: Calculate mass of isoamyl acetate

    Mass isoamyl acetate = moles isoamyl acetate * molar mas isoamyl acetate

    Mass isoamyl acetate = 0.04229 moles * 130.19 g/mol

    Mass isoamyl acetate = 5.506 grams = theoretical yield

    Step 8: Calcuate % yield

    % yield = actual yield / theoretical yield

    % yield = (4.993 / 5.506) * 100%

    % yield = 90.68 %

    The % yield is 90.68 %
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Suppose that in the synthesis of isoamyl acetate by Fisher esterification, a student began with 6.103 grams of acetic acid and 3.728 grams ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers