The empirical formula of a compound containing phosphorus and oxygen is P₂O₅.
What is the empirical formula?
The lowest whole number ratio of the components in the compound would be this.
The mass of an unknown compound is 10.15 g
The mass of phosphorus is 4.433 g.
10.15 - 4.433 = 5.717
The mass of oxygen will be 5.717g
Calculate the moles
[tex]\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}\\\\\rm Number\;of \;moles\;of\;O= \dfrac{5.717}{16}= 0.357 \\\\Number\;of \;moles\;of\;P= \dfrac{4.433 }{31}= 0.143[/tex]
Now, divide the moles by the smallest number of MOL
[tex]\dfrac{0.357 }{0.143}= 2.49 \\\\\\ \dfrac{0.143}{0.143}= 1[/tex]
Multiply the moles with 2 2.49 × 2 = 51 × 2 = 2
Thus, the empirical formula is [tex]\rm P_2O_5[/tex]
Learn more about the empirical formula
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