Respuesta :
Answer : The correct option is, (C) [tex]NiF_2[/tex]
Solution : Given,
Mass of Ni = 9.11 g
Mass of F = 5.89 g
Molar mass of Ni = 59 g/mole
Molar mass of F = 19 g/mole
Step 1 : convert given masses into moles.
Moles of Ni = [tex]\frac{\text{ given mass of Ni}}{\text{ molar mass of Ni}}= \frac{9.11g}{59g/mole}=0.15moles[/tex]
Moles of F = [tex]\frac{\text{ given mass of F}}{\text{ molar mass of F}}= \frac{5.89g}{19g/mole}=0.31moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For Ni = [tex]\frac{0.15}{0.15}=1[/tex]
For F = [tex]\frac{0.31}{0.15}=2[/tex]
The ratio of Ni : F = 1 : 2
The mole ratio of the element is represented by subscripts in empirical formula.
The Empirical formula = [tex]Ni_1F_2[/tex] = [tex]NiF_2[/tex]
Therefore, the empirical formula of a compound is, [tex]NiF_2[/tex]
