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Given the empirical formula NO with a molar mass of 59.98 g/mol, what is the molecular formula for this compound

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maacastrobr

Answer:

N₂O₂

Explanation:

The empirical formula NO tells us that the number of Nitrogen atoms will always be equal to the number of Oxygen atoms.

The molar mass of the simplest compound, NO, would be:

  • Molar Mass of NO = Molar Mass of N + Molar Mass of O = 30 g/mol

We divide the molar mass of the problem compound by the molar mass of the simplest compound:

  • 59.98 / 30 ≅ 2

This means we multiply the empirical formula times 2:

  • The molecular formula is N₂O₂
Lanuel

The molecular formula for this chemical compound (NO) is equal to 2.

Given the following data:

  • Molar mass of NO = 59.98 g/mol.

Scientific data:

  • Molar mass of oxygen (O) = 16 g/mol.
  • Molar mass of nitrogen (N) = 14 g/mol.

How to calculate molecular formula.

First of all, we would determine the gram-mass of nitrogen oxide (NO) as follows:

[tex]NO = 14+16[/tex]

NO = 30 g/mol.

For the molecular formula:

[tex](NO)n=59.98\\\\30n=59.98\\\\n=\frac{59.98}{30}[/tex]

n = 1.999 ≈ 2.0

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