In part a, you found the amount of product (3.80 mol p2o5 ) formed from the given amount of phosphorus and excess oxygen. in part b, you found the amount of product (3.40 mol p2o5 ) formed from the given amount of oxygen and excess phosphorus. now, determine how many moles of p2o5 are produced from the given amounts of phosphorus and oxygen. express your answer to three significant figures and include the appropriate units. view available hint(s)

The balanced chemical equation between phosphorus and oxygen can be given as,

3.80 mol is formed from P (limiting reactant):

Moles of P =

3.40 mol is produced when Oxygen is limiting:

Moles of =

So we have 7.6 mol P and 8.5 mol O2.

Calculating the moles of P2O5 formed from the given moles of P and O2:

Moles of phosphorus pentoxide from P =

So the moles of produced from P are

=

Moles of phosphorus pentoxide formed from O2 =

O2 produced the least amount of the product so oxygen would be the limiting reactant.

Moles of produced will be 3.40 mol

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i wish i could but this one is weird give me abc and i can solve it.