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28 April, 03:58

Consider the following reaction: A + 4B ➔ 3C + 2D If 5.0 mol of A reacts with 12.0 mol of B to form 6.0 mo! of C, the percent yield of the reaction is:

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  1. 28 April, 07:40
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    The % yiel of the reaction is 66.67%

    Explanation:

    Step 1: Data given

    Number of moles of A = 5.0 mol

    Number of moles of B = 12.0 mol

    Number of moles of C formed = 6.0 = actual yield

    Step 2: The balanced equation

    A + 4B ➔ 3C + 2D

    Step 3: Calculate the limiting reactant

    B is the limiting reactant. It will completely be consumed (12.0 moles)

    A is in excess. There will react 12/4 = 3.0 mol

    There will remain 5.0 - 3.0 = 2.0 moles

    Step 4: Calculate moles of C produced = theoretical yield

    For 1 mol of A we need 4 moles of B to produce 3 moles of C

    For12.0 moles of B we'll have 9 moles of C produced.

    Step 5: Calculate % yield

    % yield = actual yield / theoretical yield

    % yield = (6.0 mol / 9.0 mol) * 100%

    % yield = 66.67 %

    The % yiel of the reaction is 66.67%
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