Molecular Mass

# What is the empirical and molecular formulas in a compound that is 23 nitrogen and 77 oxygen and has a molecular mass of 124 gmole?

###### Answered 2007-10-02 21:08:42

The question is missing something; I must assume that the compound is 23% N by mass and 77% O by mass. Starting with NO3 as an initial guess turns up 22.6% N, 77.4% O, which agrees with the above if we round off to two significant figures. It has a molar mass of 62, precisely half the stated molecular mass. One could presume a dimer of NO3, i.e., N2O6, which is hardly a common species but does appear in the literature.

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## Related Questions

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.

Yes, nitrogen monoxide is a molecular compound with a formula of NO.

An empirical formula give information about the chemical composition of a compound. Example: tetracycline with the empirical formula C22H24N2O8 has the following composition: - carbon 59,44 % - oxygen 28,81 % - nitrogen 6,30 % - hydrogen 5,45 % If you're with plato the answer is ratios

nitrogen is an element, and nitrogen dioxide is a molecular compound.

No: The formula NO shows equal numbers of nitrogen and oxygen atoms in the compound, but the formula NO2 shows twice as many oxygen atoms as nitrogen atoms.

The empirical formula of SN has a formula unit mass of the sum of the gram atomic masses of nitrogen and sulfur, i.e., about 46.0667. The gram molecular mass given in the problem divided by this formula unit mass is about 4. Therefore, the molecular formula is S4N4.

Ammonia is a molecular compound. The hydrogen atoms share electrons with the nitrogen atom.

The empirical formula for potassium nitrate is the same as the molecular formula, KNO3, because the molecular formula shows only one atom each of potassium and nitrogen.

Ammonia and nitrogen are two distinct compounds, not a single compound that would have a molecular formula.

it can be calculated using the formula percentage composition of N =Gram molecular mass of nitrogen in the compound/ Gram molecular mass of compound *100

Divide each percentage by the atomic mass of that element. Nitrogen: 30.4 / 14 = 2.1714 Oxygen: 69.6 / 16 = 4.35 compare these and divide by the smallest, round if necessary. Nitrogen: 2.1714 / 2.1714 = 1 Oxygen: 4.35 / 2.1714 round to 2 This gives an empirical formula of NO2 The mass of this empirical formula = 14 + 2x16 = 46 Divide the molar mass by this empirical mass. 92.0 / 46 = 2 multiply the subscripts in the empirical formula by this number to get the molecular formula (NO2)2 = N2O4 THIS IS THE MOLECULAR FORMULA.

No it is ionic because when a metal (sodium) and a non-metal (nitrogen) combine it makes an ionic compound. If you combined two non-metals it would create a molecular compound.

If a compound contains an even number of nitrogen atoms (or no nitrogen atoms), its molecular ion will appear at an even mass number. If, however, a compound contains an odd number of nitrogen atoms, then its molecular ion will appear at an odd mass value. This rule is very useful for determining the nitrogen content of an unknown compound.

Yes - there are equal values of nitrogen (4) and hydrogen (12) on both sides of this equation, and all molecular formulas are in empirical form.

Nitrogen trichloride is the covalent molecular compound NCl3

Air is a molecular compound, containing large quantities of nitrogen, oxygen, and carbon dioxide.

The common name of this molecular compound is nitrogen trioxide and the systematic name is Nitrogen(III) Oxide.

Di-nitrogen tetra-hydride, but nobody calls is that.

Nitrogen Dioxide (NO2) is a molecular compound in which two oxygen molecules are bonded covalently to a central nitrogen molecule in a bent shape. The O-N-O bond angle is 134.3o as opposed to 180o due to the unbonded electron in nitrogen's outer shell. A good example of a nitrogen-based ionic compound would instead be sodium nitrate (NaNO3) or similar.

###### Elements and CompoundsChemistryNitrogenSchool SubjectsAmmoniaScienceChemical Bonding

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