If the weight of an oxide of nitrogen is 108g and 4.02g of nitrogen combine with 11.48g of oxygen to form it, what is the molecular formula of the compound

Molecular formula is N₄O₁₀

Explanation:

We are given;

Mass of the oxide of nitrogen as 108 g Mass of nitrogen as 4.02 g Mass of Oxygen is 11.48 g

We are required to calculate the molecular formula of the compound.

Step 1: Determine the number of moles of Nitrogen and Oxygen

Atomic mass of Nitrogen as 14.0 g/mol

Moles = Mass ÷ Atomic mass

Therefore;

Moles of Nitrogen = 4.02 g ÷ 14.0 g/mol

                             = 0.287 moles

Moles of Oxygen

Atomic mass of oxygen as 16.0 g/mol

Moles of Oxygen = 11.48 g ÷ 16.0 g/mol

                            = 0.7175 moles

Step 2: Determine the simplest whole number mole ratio

The mole ratio of N : O will be;

O.287 moles : 0.7175 moles

                 1 : 2.5

Multiplying by 2 , we get

                2 : 5

Therefore, the empirical formula of the nitrogen oxide is N₂O₅

Step 3: Determine the molecular formula of nitrogen oxide

Molecular formula = (empirical formula)n

Mass = 108 g

(N₂O₅)n = 108 g

((14×2) + (16 ×2))n = 108

        60n = 108

             n = 1.8

                = 2

Thus, Molecular formula = (N₂O₅)2

                                        = N₄O₁₀

Therefore, the molecular formula is N₄O₁₀

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