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.
Answers
Answer:
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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