Determine the molecular formula of a compound with an empirical formula of nh2 and a formula mass of 32.06 amu

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

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in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

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