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30 December, 20:17

8.000 moles of Cl2 (g) react with excess P4 (s) to produce 0.5741 mol of phosphorus trichloride. What is the percent yield for this reaction? P4 (s) + 6 Cl2 (g) → 4 PCl3 (l)

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  1. 30 December, 20:42
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    The percent yield is 10.77 %

    Explanation:

    Step 1: Data given

    Number of moles Cl2 = 8.00 moles

    Number of moles PCl3 produced = 0.5741 moles

    Step 2: The balanced equation

    P4 (s) + 6 Cl2 (g) → 4 PCl3 (l)

    Step 3: Calculate moles PCl3

    For 1 mol P4 we need 6 moles Cl2 to produce 4 moles PCl3

    For 8.00 moles Cl2 we'll have 4/6 * 8.00 = 5.33 moles

    Step 4: Calculate percent yield

    % yield = (actual yield / theoretical yield) * 100%

    % yield = (0.5741 / 5.33) * 100%

    % yield = 10.77%

    The percent yield is 10.77 %
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