<h3>
Answer:</h3>
Molecular formula is N₄O₁₀
<h3>
Explanation:</h3>
<u>We are given;</u>
- 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.
<h3>Step 1: Determine the number of moles of Nitrogen and Oxygen </h3>
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
<h3>Step 2: Determine the simplest whole number mole ratio</h3>
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
<h3>Step 3: Determine the molecular formula of nitrogen oxide</h3>
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
