The molecular formula of the compound has been [tex]\rm \bold{H_2O_2}[/tex].
The molecular formula of a compound has been given by the calculation of the moles of the compound by the empirical formula.
The moles of the compound has been given by:
[tex]\rm Moles\;=\;\dfrac{Mass}{Molar\;mass}[/tex]
The moles of hydrogen in 0.44 g:
[tex]\rm Moles=\dfrac{0.44}{1}\\Moles=0.44 mol[/tex]
The moles of hydrogen in the compound have been 0.44 mol.
The moles of oxygen in 6.92 gram has been:
[tex]\rm Moles=\dfrac{6.92}{16}\\Moles=0.44 mol[/tex]
The moles of oxygen in the compound have been 0.44 mol.
The moles have been equal thus the empirical formula of the compound has been OH.
The mass of the compound has been 34 g/mol.
The mass of the empirical formula has been 17 g.
The formula unit of empirical formula has been:
[tex]\rm Formula\;unit=\dfrac{34}{17} \\ Formula\;unit=2[/tex]
The molecular formula of the compound has been [tex]\rm \bold{H_2O_2}[/tex].
For more information about molecular formulas, refer to the link:
https://brainly.com/question/1247523
