Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula

The molecular formula is N2H4O4.

Explanation:

Assume 100 g of this compound  

mass N = 29.17 g

mass H = 4.20 g

mass O = 66.63 g  

moles N = 29.17 g/ 14.0067 g/mol = 2.083

moles H = 4.20 g/ 1.008 g/mol = 4.16

moles O = 66.63 g/ 15.999 g/mol = 4.16

The smallest number is divided to get the ratio as N:H:O

                -----> H and O

                  -----> N  

the empirical formula is calculated as NH2O2 ( molar mass = 48.03 g/mol)

96.04 / 48.03 = 2

By  multiplying the empirical formula by 2, we get

The molecular formula is N2H4O4.

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.

explanation: