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# What is the Molar mass of empirical formula NO2?

Updated: 8/9/2023 Wiki User

11y ago

The empirical mass of NO is 14 + 16 = 30

Divide 138 / 30 ~ = 4.5.

The fact that the numbers are not whole number would suggest that the empirical formula is incorrect.

However, if we use say NO2 as the empirical formula , then the empirical mass is 14 + 16 + 16 = 46

divide 138 /46 = 3

So NO2 has a formula of N3O6 . This substance does not exist, So it would suggest that the formula is 3NO2 (3/2)N2O4 .

I would suggest that the original empirical formula is incorrect. and that the substance is either nitrogen dioxide (NO2) or dinitrogen tetroxide N2O4. lenpollock

Lvl 14
5mo ago   Wiki User

12y ago

The formula of NO2 has a molecular weight of 46 g/mol. Your compound has a molecular weight of 92 g/mol. As you can see the molecular weight of the compound is twice that of the empirical formula. Therefore the molecular formula of your compound is:

2 *(NO2) ---> N2O4   Wiki User

6y ago

Ar of N = 14g/mol Ar of O = 16g/mol

Mr of NO2 = 14+2(16) = 46g/mol

Mr of NxO2x = 138.02g/mol

(Mr of NxO2x / Mr of NO2) = 138.02/46 = 3.000434783 = 3 Therefore x = 3 and the molecular formula is N3O2(3) = N3O6 (but this compound is only hypothetical)   Wiki User

10y ago

The molecular formula is the same as the empirical formula, NO2. The compound NO2 has a molar mass of 46g/mol, so the empirical and molecular formulas are the same.   Wiki User

8y ago

The molecular formula is N2o4.   Wiki User

11y ago

92 g   Wiki User

10y ago

N3o6   Earn +20 pts  