When Phosphorus is ignited in air or oxygen, it burns with a yellow flame to form a white smoke. Here is the equation of this reaction from my chemistry text book:
P4(s) + 3O2(g) -> P4O6 (s)
I am wondering why a Phosphorus molecule needs three oxygen molecule to react. Why one Phosphorus molecule can not react with one oxygen molecule and form one P3O2 molecule:
P4(s) + O2(g) -> P4O2
This equation is perfectly balanced and makes sense. Why it is not considered? Do we use the first formula because for reacting a molecule of P4 we necessarily need three O2? Or there is another reason behind it?
P4(s) + 3O2(g) -> P4O6 (s)
I am wondering why a Phosphorus molecule needs three oxygen molecule to react. Why one Phosphorus molecule can not react with one oxygen molecule and form one P3O2 molecule:
P4(s) + O2(g) -> P4O2
This equation is perfectly balanced and makes sense. Why it is not considered? Do we use the first formula because for reacting a molecule of P4 we necessarily need three O2? Or there is another reason behind it?