A certain organic compound in the vapor state has a density of 3.27 g/L at 95°C and 758 torr...?

A certain organic compound in the vapor state has a density of 3.27 g/L at 95°C and 758 torr. What is the molecular weight? If the compound contains 24.2% C, 4.1% H, and 71.7% Cl, what is the molecular formula?

Answer:
we can use the formula
d = M p /RT

M = d RT / p

p = 758 / 760 = 0. 997 atm
T = 95 + 273 = 368 K

M = 3.27 x 0.0821 x 368 / 0.997 = 99.1 g/mol

We consider 100 g of this compound : we have 24.2 g of C , 4.1 g of H and 71.7 g of Cl

24.2 / 12.011 =2.01 moles C
4.1 / 1.00794 = 4.07 moles H
71.7 / 35.453 = 2.02 moles Cl

we divide for the smallest number and we get the empirical formula
C H2Cl ( mass = 51 g/mol)
99.1 / 51 = 1.9

the molecular formula is
C2H4Cl2
may be CH3CHCl2 or CH2ClCH2Cl

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