Question #168e9

1 Answer
Oct 1, 2015

6.49xx10^(-2)mol(O_2)

Explanation:

The reaction is:
P_4(s) + 3O_2(g) -> P_4O_6(s)

We should calculate first the number of mole of P_4O_6(s):
n=m/(MM) =(4.76cancel(g))/(219.88cancel(g)/(mol))=2.16xx10^(-2) mol

The number of mole of oxygen needed to produce 4.76g of P_4O_6(s):

n_(O_2)=2.16xx10^(-2)cancel(mol(P_4O_6))xx(3 mol(O_2))/(1 cancel(mol(P_4O_6)))
=6.49xx10^(-2)mol(O_2)