Question

Phosphorus reacts with oxygen to form diphosphorus pentoxide, P,Os. 4P(s) + 50,(8) - 2P,0,() How many grams of P, O, are formed when 3.11 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots. 3.113 px ( ) ( ) ( ) g Pos Answer Bank 1 mol O, 1 mol P 4 mol P 141.94 g P,0, 2 mol P,0 5 mol O, 1 mol P,0 30.97 g 32.00 g 0.

Answer 1

Molar mass of P = 30.97 g/mol

mass of P = 3.11 g

mol of P = (mass)/(molar mass)

= 3.11/30.97

= 0.1004 mol

According to balanced equation

mol of P2O5 formed = (2/4)* moles of P

= (2/4)*0.1004

= 5.021*10^-2 mol

Molar mass of P2O5,

MM = 2*MM(P) + 5*MM(O)

= 2*30.97 + 5*16.0

= 141.94 g/mol

mass of P2O5 = number of mol * molar mass

= 5.021*10^-2*1.419*10^2

= 7.127 g

Answer: 7.13 g

I mol P 2 mol P,O, 141.94 g P,O, 3.11 g PX [ 7.13 7.13 8P,Os 30.97 g P 4 mol P 1 mol P,03 Answer Bank 1 mol O, 1 mol P 4 mol P 141948 P,0; 2 mol P,05 5 mol O2 1 mol P,O, 30.97 g P 32.00 g 0,