Question

An organic compound containing oxygen, carbon, hydrogen and nitrogen contains 20 % carbon, 6.7 % hydrogen and 46. 67 % nitrogen. Its molecular mass was found to be 60 g mol^ -1. Find the molecular formula of the compound. ​

Answer 1

Answer:

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Answer 2

Given :-

• Carbon =20 %

• Hydrogen = 6.7 %

• Nitrogen = 46.67 %

• Oxygen = 100 - ( 20 + 6.7 + 46.67 ) = 100 - 73.37  = 26.63 %
• Molar mass = 60 g

Solution :-

Relative no of atoms

First we need to divide the % composition of the elements with the atomic masses of the elements

Carbon

C = 20 / 12 = 1.66

Hydrogen

H = 6.7 /1 = 6.7

Nitrogen

N = 46.67 / 14 = 3.33

Oxygen

O = 26.63 / 16 = 2

Simple ratio

Divide all the values obtained above by the smallest value obtained( i.e 1.66) in this case

Carbon

C  = 1.66 / 1.66 = 1

Hydrogen

H = 6.7 /1.66 = 4

Nitrogen

N  = 3.33 / 1.66 = 2

Oxygen

O = 2 / 1.66 = 1

⟹ Empirical formula = CH4 N2 O

⟹ Empirical mass = C + 4 (H) + 2(N) + O

⟹ Empirical mass = 12 + 4 (1) + 2(14) + 16

⟹ Empirical mass = 12 + 4  + 28 + 16

⟹ Empirical mass = 60 g

⟹ Molecular mass = Empirical mass = 60 g

⟹ Molecular formula = Empirical formula =  CH4 N2 O

Molecular formula of the compound =  CH4 N2 O