“analysis of a compound of phosphorus nitrogen and chlorine show that it is 26.73% p and 12.09% n with cl accounting for the remainder. in a separate experiment, the molar mass of the compound was found to be 463.5 g/mol. determine the molecular formula of the compound.” !

The molecular formula will be=

Explanation:

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of P = 26.73 g

Mass of N = 12.09 g

Mass of Cl = (100-12.09) g  = 61.18 g

Step 1 : convert given masses into moles.

Moles of P =

Moles of N =

Moles of Cl =

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For P =

For N =

For Cl =

The ratio of P: N: Cl = 1: 1: 2

Hence the empirical formula is

The empirical weight of = 1(31)+1(14)+2(35.5)= 116 g.

The molecular weight = 463.5 g/mole

Now we have to calculate the molecular formula:

The molecular formula will be=

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