Answer: The empirical formula is [tex]FeS[/tex]
Explanation:
Mass of Fe = 3.78 g
Mass of S = (5.95-3.78) g = 2.17 g
Step 1 : convert given masses into moles.
Moles of Fe =[tex]\frac{\text{ given mass of Fe}}{\text{ molar mass of Fe}}= \frac{3.78g}{56g/mole}=0.0675moles[/tex]
Moles of S = [tex]\frac{\text{ given mass of S}}{\text{ molar mass of S}}= \frac{2.17g}{32g/mole}=0.0678moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For Fe = [tex]\frac{0.0675}{0.0675}=1[/tex]
For S =[tex]\frac{0.0678}{0.0675}=1[/tex]
The ratio of Fe : S= 1: 1
Hence the empirical formula is [tex]FeS[/tex]
