A compound contains `4.07% H,. 24.27% C`, and `71.65% Cl`. If its molar mass is `98.96`, the molecular formula will be

Options

A. CHCl
B. `CH_(3)Cl`
C. `C_(2)H_(4)Cl_(2)`
D. `C_(2)HCl`

Answer

C

Explanation

Let us assume 100 g of compound contains `4.07` g H,
`24.27` g C and `71. 65` g Cl.
Number of moles of `"H" = (4.07)/1=4.07`
Number of moles of `"C" = (24.27)/12=2.02`
Number of moles of `"Cl"=(71.65)/35.5=2.02`
Ratio of H : C : Cl : is 4 : 2 : 2 or 2 : 1 : 1
`because` Its empirical formula is `CH_(2)Cl`.
Now, we have
`n=("Molecular formula weight")/("Empirical formule weight") `
`=(98.96)/49.5=2`
`therefore` Molecular formula `=nxx ("empirical formula")`
`=2xx(CH_(2)Cl)`
`=C_(2)H_(4)Cl_(2)`