Question

An organic compound containing oxygen,hydrogen,carbon and nitrogen contains 20% carbon,6.7%hydrogen and 46.67 nitrogen. Its molecular mass found is 16.find the molecular formula of the compound.​

Answer 1

percentage weight of C = 20%

percentage weight of H = 6.7%

percentage weight of N = 46.67%

so, percentage weight of O = 100 - (20 + 6.7 + 46.67) = 26.63 %

finding percentage - mass value of each atom.

for oxygen, O ⇒ 26.63/16 ≈ 1.66

for hydrogen, H ⇒ 6.7/1 = 6.7

for carbon, C ⇒20/12 = 5/3 ≈ 1.66

for nitrogen , N = 46.67/14 ≈ 3.33

finding simple ratio of (percentage-mass)

i.e., O : H : C : N = 1 : 4 : 1 : 2

so, empirical formula will be $CH_4N_2O$

given, molecular mass = 60 [ you did mistake in typing ]

so, 60 = n × (12 + 4 + 2 × 14 + 16)

n = 1

hence, molecular formula is $n(CH_4N_2O)$ = $CH_4N_2O$

Answer 2

Answer:

see the attachment ✌️❣️