A compound contains `4.07% H,. 24.27% C`, and `71.65% Cl`. If its molar mass is `98.96`, the molecular formula will beA. CHClB. `CH_(3)Cl`C. `C_(2)H_(4)Cl_(2)`D. `C_(2)HCl`

A compound contains `4.07% H,. 24.27% C`, and `71.65% Cl`. If its mola

1.	A compound contains `4.07% H,. 24.27% C`, and `71.65% Cl`. If its molar mass is `98.96`, the molecular formula will beA. CHClB. `CH_(3)Cl`C. `C_(2)H_(4)Cl_(2)`D. `C_(2)HCl`
Answer» Correct Answer - C 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)`

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A compound contains `4.07% H,. 24.27% C`, and `71.65% Cl`. If its molar mass is `98.96`, the molecular formula will beA. CHClB. `CH_(3)Cl`C. `C_(2)H_(4)Cl_(2)`D. `C_(2)HCl`

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