Question

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Phosphorus reacts with oxygen to form diphosphorus pentoxide, P,Os 4 P(s)+50,(g) 2 P,Og(s) How many grams of P,O, are formed when 5.65 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. 5.65 g Px g P,O Answer Bank 141.94 g P,O, 2 mol P,O 1 mol O, 1 mol P,O, I mol P 32.00 g O, 30.97 g P 4 mol P 5 mol O

Answer 1

Molar mass of P = 30.97 g/mol

mass of P = 5.65 g
mol of P = (mass)/(molar mass)
= 5.65/30.97
= 0.1824 mol



According to balanced equation
mol of P2O5 formed = (2/4)* moles of P
= (2/4)*0.1824
= 9.122*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
= 9.122*10^-2*1.419*10^2
= 12.95 g
Answer: 13.0 g

2 mol P,O 1 mol P 141.94 g P,O 5.65 g Px g P,Os 13.0 1 mol P,O 4 mol P 30.97 g P