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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.

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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

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)

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.

The molecular formula is N2o4.

92 g

N3o6

Q: What is the Molar mass of empirical formula NO2?

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Determine the molar mass of NO2 using the subscripts in the formula and the atomic weights in grams from the periodic table. 1 mole NO2 = (1 x 14.0067g N) + (2 x 15.9994g O) = 46.0055g NO2 Calculate the moles NO2 by dividing the given mass by the molar mass. 25.5g NO2 x (1mol NO2/46.0055g NO2) = 0.554mol NO2

N= 7 O = 16 Molar mass = 39

46 grams XP!

NO2 and N2O4

Assume those percentages as mass. Find moles. 30 grams Nitrogen (1 mole N/14.01 grams) = 2.141 moles ( call it 2 ) 70 grams oxygen (1 mole O/16.0 grams) = 4.4 moles ( call it 4 ) smallest mole number is 1 in formula and divide larger number by it 2/4 = 2 so.............. NO2 nitrogen dioxide is the empirical formula

Related questions

46.0055. The formula for Nitrogen dioxide is NO2

Determine the molar mass of NO2 using the subscripts in the formula and the atomic weights in grams from the periodic table. 1 mole NO2 = (1 x 14.0067g N) + (2 x 15.9994g O) = 46.0055g NO2 Calculate the moles NO2 by dividing the given mass by the molar mass. 25.5g NO2 x (1mol NO2/46.0055g NO2) = 0.554mol NO2

N= 7 O = 16 Molar mass = 39

NO2 is 46 molar mass

46 grams XP!

NO2 and N2O4

Sn(NO2)4

The empirical formula for nitrogen dioxide is the same as its molecular formula - NO2. See related question below for more details on how to find empirical formulas.

Assume those percentages as mass. Find moles. 30 grams Nitrogen (1 mole N/14.01 grams) = 2.141 moles ( call it 2 ) 70 grams oxygen (1 mole O/16.0 grams) = 4.4 moles ( call it 4 ) smallest mole number is 1 in formula and divide larger number by it 2/4 = 2 so.............. NO2 nitrogen dioxide is the empirical formula

196.9497 g/mol

The molar mass of nitrogen dioxide is: 1 N + 2 O. M= 14,007 + (2 x 15,999) = 46 g

The chemical formula for Barium Nitrite is Ba(NO2)2. Ba = Barium N = Nitrogen O = Oxygen Its molar mass is 229.338 g/mol.