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15 May, 15:36

an experiment reacts 21 grams of zinc metal with a solution of iron 3 sulphate. after the reaction, 10.8 grams of iron metal are recovered. what is the percent yield of the experiment?

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  1. 15 May, 15:43
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    90.38%

    Explanation:

    We are given;

    Mass of Zinc metal is 21 g Mass of Iron metal produced is 10.8 g

    We are required to calculate the percent yield of the experiment;

    Step 1: Write the balanced equation for the reaction.

    The balanced equation for the reaction is given by;

    3Zn + Fe₂ (SO₄) ₃ → 3ZnSO₄ + 2Fe

    Step 2: Moles of Zinc metal used

    We know that, moles = Mass : Molar mass

    Molar mass of Zn is 65.38 g/mol

    Therefore;

    Moles of Zn = 21 g : 65.38 g/mol

    = 0.321 moles

    Step 2: Moles of Fe produced From the equation;

    3 moles of Zinc metal reacts to yield 2 moles of iron metal

    Therefore; Moles of Iron = Moles of Zinc * 2/3

    = 0.321 moles * 2/3

    = 0.214 mol

    Step 3: Theoretical yield of the reaction

    Theoretical mass of Iron metal produced

    Mass = Number of moles * Molar mass

    Molar mass of iron is 55.845 g/mol

    Thus, mass of Iron = 0.214 mol * 55.845 g/mol

    = 11.95 g

    Step 4: Percent yield of the experiment

    % yield = (Actual yield : theoretical yield) * 100

    Therefore;

    % yield = (10.8 g : 11.95 g) * 100

    = 90.38%

    Thus, the % yield of the experiment is 90.38%
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