In Part A, you found the number of moles of product (1.80 mol P2O5 ) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the number of moles of product (1.40 mol P2O5 ) formed from the given amount of oxygen and excess phosphorus. Now, determine the number of moles of P2O5 is produced from the given amounts of phosphorus and oxygen

1.40 moles.

Explanation:

The balanced chemical equation for the reaction of Phosphorus and Oxygen is as follows -

In Part A, the oxygen was taken in excess. So Phosphorus will be the limiting reagent.

Since, 2 moles of is formed by 4 moles of

So, for 1.8 moles of   amount of required moles of =

In Part B, the phosphorus was taken in excess so oxygen will be the limiting reagent.

Since, 2 moles of is formed by 5 moles of oxygen

So, for 1.40 moles of moles of required =

Thus as of now we have 3.60 moles of and 3.50 moles of .

As in the reaction of formation of , oxygen is the limiting reagent.

So the moles of formed by the 3.50 moles of oxygen will be

= = 1.40 moles.

thats how its supposed to be

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