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

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