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A sample was decomposed in the laboratory and found to have 38.67g C, 16.22g H, and 45.11g N.?
A sample was decomposed in the laboratory and found to have 38.67g C, 16.22g H, and 45.11g N.
a)Find the molecular formula of this compound if the Formula mass is 62.12 g/mole.
b)Determine how many H atoms would be in a 3.50g sample of this compound
1 Answer
- 9 years agoFavorite Answer
a)
Element-------C---------H-------N
No.of mol--3.222---16.22---3.222
Ratio = 1: 5: 1
Empirical formula: CH5N
n: 62.12/ (12+5+14) = 2
Molecular formula = C2H10N2
b)
Mass of H = fraction of H x mass of sample
So, (10x1)/62.12 x 3.50g = 0.563g (3s.f.)
Edit: My answer was cut off. ):
Hope this helps! :))
