Answer : The empirical formula of the compound is, [tex]OF_2[/tex]
Solution : Given,
If percentage are given then we are taking total mass is 100 grams.
So, the mass of each element is equal to the percentage given.
Mass of O = 29.6 g
Mass of F = 70.4 g
Molar mass of F = 19 g/mole
Molar mass of O = 16 g/mole
Step 1 : convert given masses into moles.
Moles of O = [tex]\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{29.6g}{16g/mole}=1.85moles[/tex]
Moles of F = [tex]\frac{\text{ given mass of F}}{\text{ molar mass of F}}= \frac{70.4g}{19g/mole}=3.70moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For O = [tex]\frac{1.85}{1.85}=1[/tex]
For F = [tex]\frac{3.70}{1.85}=2[/tex]
The ratio of O : F = 1 : 2
The mole ratio of the element is represented by subscripts in empirical formula.
The Empirical formula = [tex]O_1F_2=OF_2[/tex]
Therefore, the empirical formula of the compound is, [tex]OF_2[/tex]
