Question

A compound contains carbon 14.4 hydrogen 1.2 and chlorine

Answer 1

Hey here is your answer....

A compound contains carbon 14.4 %, hydrogen 1.2 % and chlorine 84.5 %. The relative molecular mass of this compound is 168, its molecular formula is:[C=12,H=1,Cl=35.5]

A C2H2Cl3

B C2H4Cl4

C CH2Cl4

D C2H2Cl4

Solution

Element % composition Atomic weight Relative No. of atoms Simplest ratio

Carbon 14.4 12 14.4/12 = 1.2 1.2/1.2 = 1

Hydrogen 1.2 1 1.2/1 = 1.2 1.2/1.2 = 1

Chlorine 84.5 35.5 84.5/35.5 = 2.38 2.38/1.2 = 2

Hence, empirical formula is CHCl2.

n = Molecular mass/Empirical formula mass

= 168/(12 + 1 + 70)

= 168/83

= 2.

Therefore, molecular formula =(CHCl2)×2=C2H2Cl4.

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Answer 2

C=12

H=1

Cl=35.5

Relative no of atoms is=14.4/12

Rel. no. Of. Atoms =1.2/1

Rel. no. Of atoms =84.5/35.5

Therefore empirical formula=CHCl2

Molecular mass/empirical mass=n

n=168/83

n=2

Therefore empirical formula *2= C2H2CL4