Question

Determine the molecular formula of a compound with an empirical formula of NH2 and a formula mass of 32.06 amu

Answer 1

N2H4

Each nitrogen weighs 14.01 and each H weighs 1.01. !4.01+14.01+1.01+1.01 = 32.06 (roughly) 

Answer 2

Answer:N2H4

Explanation: Empirical Formula, EF= NH2

Mass of the EF = mass of Nitrogen + mass of Hydrogen

EF = 14.007 + 1.008

= 15.015

Then, divide the given formula mass by the EF. That is,

32.06/15.015 = 2.135 = 2 (to the nearest whole number) ......... (1)

To get the molecular formula, multiple the empirical formula with the number from the equ (1) above.

Molecular formula = 2[NH2] = N2H4