Answer: The maximum number of moles of [tex]P_2O_5[/tex] theoretically made is 2.194 moles.
Explanation:
To calculate the number of moles, we use the equation
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of [tex]P_4[/tex] = 136 g
Molar mass of [tex]P_4[/tex] = 123.9 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of }P_4=\frac{136g}{123.9g/mol}=1.097mol[/tex]
The chemical equation for the formation of [tex]P_2O_5[/tex] follows:
[tex]P_4+5O_2\rightarrow 2P_2O_5[/tex]
Oxygen is present in excess, so it is considered as an excess reagent.
[tex]P_4[/tex] is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
If 1 mole of [tex]P_4[/tex] is producing 2 moles of [tex]P_2O_5[/tex]
So, 1.097 moles of [tex]P_4[/tex] will produce = [tex]\frac{2}[1}\times 1.097=2.194mol[/tex] of [tex]P_2O_5[/tex]
Hence, the maximum number of moles of [tex]P_2O_5[/tex] theoretically made is 2.194 moles.
