Acompound was found to contain 10.06% carbon, 89.10% chlorine, and 0.84% hydrogen, by mass. if the molar mass of the compound was found to be 119.6 g/mol, its molecular formula will be

Answer : The molecular formula of a compound is,

Solution :

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 C = 0.1006 g

Mass of H = 0.0084 g

Mass of Cl = 0.8910 g

Molar mass of C = 12 g/mole

Molar mass of H = 1 g/mole

Molar mass of Cl = 35.5 g/mole

Step 1 : convert given masses into moles.

Moles of C =

Moles of H =

Moles of Cl =

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

For C =

For H =

For Cl =

The ratio of C : H : Cl = 1 : 1 : 3

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula =

The empirical formula weight = 1(12) + 1(1) + 3(35.5) = 119.5 gram/eq

Now we have to calculate the molecular formula of the compound.

Formula used :

Molecular formula =

Therefore, the molecular of the compound is,

particle   p is an electron and particle q is a neutron

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