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24 November, 03:08

When heated, lithium reacts with nitrogen to form lithium nitride: 6Li (s) + N2 (g) → 2Li3N (s) What is the theoretical yield of Li3N in grams when 12.7 g of Li is heated with 34.7 g of N2? g If the actual yield of Li3N is 5.85 g, what is the percent yield of the reaction? %

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  1. 24 November, 03:14
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    The % yield of the reaction = 27.5 %

    Explanation:

    Step 1: Data given

    Mass of Li = 12.7 grams

    Mass of N2 = 34.7 grams

    Actual yield of Li3N = 5.85 grams

    Molar mass of Lithium = 6.94 g/mol

    Molar mass of N2 = 28 g/mol

    Molar mass of LI3N = 34.83 g/mol

    Step 2: The balanced equation:

    6Li (s) + N2 (g) → 2Li3N (s)

    Step 3: Calculate moles of Lithium

    Moles Li = mass Li / Molar mass Li

    Moles Li = 12.7 grams / 6.94 g/mol

    Moles Li = 1.83 moles

    Step 4: Calculate moles of N2

    Moles N2 = 34.7 g / 28 g/mol

    Moles N2 = 1.24 moles

    Step 5: Limiting reactant

    For 6 moles Li consumed, we need 1 mole of N2 to produce 2 moles of Li3N

    Lithium is the limiting reactant. It will completely be consumed (1.83 moles).

    N2 is in excess. There will be consumed 1.83 / 6 = 0.305 moles

    There will remain 1.24 - 0.305 = 0.935 moles

    Step 6: Calculate moles of Li3N

    For 6 moles Li consumed, we need 1 mole of N2 to produce 2 moles of Li3N

    For 1.83 moles Li, we'll have 1.83/3 = 0.61 moles of Li3N

    Step 7: Calculate mass of Li3N

    Mass Li3N = moles LI3N * Molar Mass LI3N

    Mass Li3N = 0.610 moles * 34.83 g/mol

    Mass Li3N = 21.2463 grams = Theoretical yield

    Step 8: Calculate % yield

    % yield = actual yield / theoretical yield

    % yield = (5.85 / 21.2463) * 100% = 27.5%

    The % yield of the reaction = 27.5 %
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