White phosphorus reacts with chlorine and the product hydrolyses in the presence of water. Calcualte the mass of HCl obtained by the hydrolysis of the product formed by the reaction of 62 g of white phosphorus with chlorine in the presence of water.

Explanation

The chemical reactions involved are :
`P_(4)+6Cl_(2) to 4PCl_(3)`
`(PCl_(3)+3H_(2)O to H_(3)PO_(3)+3HClxx4)/(underset(1 mol)(P_(4))6Cl_(2)+12H_(2)O to 4H_(3)PO_(3)+ underset(12 mol)(12HCl))`
No. of moles in 62 g of white phosphorus `=("Mass of " P_(4))/("Molar mass")=((62g ))/((124 " g mol"^(-1)))=0.5 mol`
1.0 mole of white phosphorus `(P_(4))` forms HCl=12 mol
0.5 mole of white phosphorus `(P_(4))` forms HCl `=12xx0.5=6` mol
Mass of HCl formed `=(6 mol)xx(36.5 "g mol"^(-1))=219 g`