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29 November, 09:20

What mass of pcl5 will be produced from the given masses of 26.0 g of p4 and 50.0 g of cl2?

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  1. 29 November, 12:27
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    The balanced chemical reaction for the above reaction is as follows;

    P₄ + 10Cl₂ - - > 4PCl₅

    stoichiometry of P₄ to Cl₂ is 1:10

    we need to first find the limiting reactant of the reaction,

    number of P₄ moles - 26.0 g / 124 g/mol = 0.210 mol

    number of Cl₂ moles - 50.0 g / 70.9 g/mol = 0.705 mol

    if P₄ is limiting reactant,

    then if 1 mol of P₄ reacts with 10 mol of Cl₂

    then 0.210 mol of P₄ reacts with 10x 0.210 = 2.10 mol of Cl₂

    but only 0.705 mol of Cl₂ is present, therefore Cl₂ is the limiting reactant.

    stoichiometry of Cl₂ to PCl₅ is 10:4

    if 10 mol of Cl₂ produces 4 mol of PCl₅

    then 0.705 mol of Cl₂ produces - 4/10 x 0.705 = 0.282 mol of PCl₅

    Mass of PCl₅ produced - 0.282 mol x 208.25 g/mol = 58.7 g produced
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