[nebbzlol]

Question: A sample of a compound of N and O reacts with excess H2 (g) to give 0.123g of NH3 and 0.325g of H2O. Determine the empirical formula of this compound.


Would I use % composition to solve this or mole ratio?

I got stuck doing mole ratio because I don't know the molecular mass of the compound of N and O to find the mass of the compound and the moles (coefficient of each reactant and product).

Using % composition I tried assuming that the percent composition of N on the left side of all the reactants would equal to the % composition of N of all products. That didn't work either.

[AWK]

Using percent composition correctly should give also empirical formula, but this is a longest way.

Hint: calculate moles of N and O in ammonia and water.

[nebbzlol]

Using percent composition correctly should give also empirical formula, but this is a longest way.

Hint: calculate moles of N and O in ammonia and water.

Would the moles of N in ammonia be equal to the moles of N in the unknown compound?

[Burner]

Would the moles of N in ammonia be equal to the moles of N in the unknown compound?

Yes

[Borek]

Determine the empirical formula of this compound.

Do you know what the empirical formula is, and how it differs from the molecular formula?