A carbon compound contains $4.07$ , $24.27$ , $71.6$ . Its molar mass is $98.96 g {m o l}^{- 1}$ , What are its empirical and molecular formulae ?

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Solution

Compound contains $4.07 %$ hydrogen $24.97 %$
carbon and $71.65 %$ chlorine
Let amount of amount be $100 g$
amount of hydrogen $= 4.07 g$
amount of carbon $= 24.27 g$
amount of chlorine $= 71.65 g$
number of mole of hydrogen $= \frac{4.07}{1} = 4.07$
Number of mole of carbon $= \frac{24.27}{12} = 2.0225$
Number of mole of chlorine $= 2.0183$
$2.0225 : 4.07 : 2.0183$
$3 : 2 : 2$
$C H_{2} C l$
Empirical formula mass $= 12 + 2 + 35.5$
$= 49.5$
$n = \frac{M o l a r m a s}{E m p i r i c a l f o r m u l a m a s s} = \frac{98.96}{49.5}$
$= 2$
Molecular formula $= C_{2} H_{4} C l_{2}$

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