The molecular formula of the compound is
[tex]N _{2}O _{4}.[/tex]
The empirical formula of the compound is,
[tex] \frac{30.4 \: g}{14.01 \: g \: mol^{ - 1} } = 2.17 \: mol \:of \: N[/tex]
[tex]\frac{69.6 \: g}{16.0 \: g \: mol^{ - 1} } = 4.35\: mol \: of \: O[/tex]
In the compound, 2.17 moles of Nitrogen are present.
In the compound, 4.35 moles of oxygen are present.
The empirical formula of the compound is
[tex]NO _{2}.[/tex]
The molecular formula of the compound is,
[tex]Molecular \: Formula = (EF) _{n}[/tex]
[tex] = 2 \times (14.01 + 2 \times 16.00) \: g \: mol ^{ - 1} [/tex]
n = 2
[tex]The \: molecular \: formula \: is \: N _{2}O _{4}[/tex]
and the compound is dinitrogen tetroxide. It is the dimer of nitrogen dioxide.
Therefore, the molecular formula of the compound is
[tex]N _{2}O _{4}.[/tex]
To know more about dimer, refer to the below link:
https://brainly.com/question/13312552
#SPJ4
