What is the empirical formula for a compound containing 38.8% carbon C 16.2% hydrogen H and 45.1% nitrogen N )? Ar C 12 H 1 N 14?

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The empirical formula of a compound represents the simplest whole number ratio of elements in the compound.

We must first determine the moles of each element in the compound by dividing the given mass by the molar mass.

Since the masses of all of the elements equal #"100.1 g"#, we can use the masses as given.

#"mol C":# #(38.8"g C")/(12.011"g"/"mol")="3.23 mol"#

#"mol H":# #(16.2"g H")/(1.008"g"/"mol")="16.1 mol"#

#"mol N":# #(45.1"g N")/(14.007"g"/"mol")="3.22 mol"#

To determine the subscripts of the empirical formula, we find the lowest whole number ratio for each element by dividing the moles of each element by the least number of moles, in this case #"3.22 mol"#.

#"C":# #(3.23)/(3.22)=1.00#

#"H":# #(16.1)/(3.22)=5.00#

#"N":# #(3.22)/(3.22)=1.00#

The empirical formula is #"CH"_5"N"#.

Note: If the mol ratios are not all whole numbers, you will need to multiply each mole ratio by the same factor that will make all mol ratios whole numbers.

This may be methylamine, #"CH"_3"NH"_2#, derived from ammonia, #"NH"_3"#, in which one #"H"# atom is replaced by a methyl group #"-CH"_3"#. However, we can't know this for certain unless we are given the molecular mass.