Respuesta :
Answer:
1.40 moles.
Explanation:
The balanced chemical equation for the reaction of Phosphorus and Oxygen is as follows -
[tex]4P + 5O_2 = 2P_2O_5[/tex]
In Part A, the oxygen was taken in excess. So Phosphorus will be the limiting reagent.
Since, 2 moles of [tex]P_2O_5[/tex] is formed by 4 moles of [tex]P[/tex]
So, for 1.8 moles of [tex]P_2O_5[/tex] amount of required moles of [tex]P[/tex] = [tex]\frac{4}{2} \times 1.80 = 3.60[/tex]
In Part B, the phosphorus was taken in excess so oxygen will be the limiting reagent.
Since, 2 moles of [tex]P_2O_5[/tex] is formed by 5 moles of oxygen
So, for 1.40 moles of [tex]P_2O_5[/tex] moles of [tex]O_2[/tex] required = [tex]\frac{5}{2} \times 1.40 = 3.50[/tex]
Thus as of now we have 3.60 moles of [tex]P_2O_5[/tex] and 3.50 moles of [tex]O_2[/tex].
As in the reaction of formation of [tex]P_2O_5[/tex], oxygen is the limiting reagent.
So the moles of [tex]P_2O_5[/tex] formed by the 3.50 moles of oxygen will be
[tex]P_2O_5[/tex] = [tex]\frac{2}{5} \times 3.50[/tex] = 1.40 moles.
