Answer:
D 4P +3O₂ → 2 P₂O₃
Explanation:
In this problem, we need to convert the mass of phosphorus and oxygen to moles trying to find the ratio of reaction (The moles of P that reacts per mole of O₂):
Moles P:
12.4g P * (1mol P / 31g) = 0.4 moles
Moles O₂:
9.6g * (1mol / 32g) = 0.3 moles
The ratio of reaction is:
0.4 mol / 0.3 mol = 1.33 = 4 moles of P / 3 moles of O₂
That means 4 moles of P react with 3 moles of O₂ and the reaction that represents this ratio is:
The reaction of 12.4 g Phosphorous with 9.6 grams of Oxygen will be represented as [tex]\rm 4\;P\;+\;3\;O_2\;\rightarrow\;2\;P_2O_3[/tex]
In a chemical equation, the stoichiometric values are the moles of the molecules involved in the reaction. For the reaction of Phosphorous and oxygen, the moles of both elements are to be calculated.
Moles = [tex]\rm \frac{weight}{molecular\;weight}[/tex]
Moles of Phosphorous = [tex]\rm \frac{12.4}{31}[/tex]
Moles of Phosphorous = 0.4
Moles of oxygen = [tex]\rm \frac{9.6}{16}[/tex]
Moles of oxygen = 0.6
Moles of [tex]\rm O_2[/tex] = 0.3
The equation will be:
[tex]\rm 0.4\;P\;+\;0.3\;O_2\;\rightarrow\;2\;P_2O_3[/tex]
[tex]\rm 4\;P\;+\;3\;O_2\;\rightarrow\;2\;P_2O_3[/tex]
The correct reaction will be D.
For more information about the chemical equation, refer the link:
https://brainly.com/question/1689737?referrer=searchResults
