Question #168e9

1 Answer
Dr. Hayek
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)#

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