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Determine the molecular formula of a compound whose molecular mass is 60.00 g/mol and has an empirical formula of ch4n. ch4n c2h5n2 c2h8n2 c3h12n3

Sagot :

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

Learn more about the Molecular formula with the help of the given link:

https://brainly.com/question/14425592

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