Molecular formula of a compound whose molecular mass is 60.00 g/mol and has an empirical formula of C₂H₈N₂.
We know the empirical formula and thus the molar mass of the empirical formula, we simply need to find out how many of these fit into the molar mass of the molecular formula.
In this problem, we have an empirical formula of CH₄N
so the molar mass is 12 + 4 + 14 = 30 g/mol.
Molecular formula mass/Empirical formula mass=60 g/mol/30 g/mol=2
The molecular formula is TWICE that of the empirical formula.
Molecular formula = 2XCH₄N = C₂H₈N₂
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