Compound consists of carbon, hydrogen and fluorine. In one experiment, combustion of 2.50 g of the compound produced 3.926 g of CO2. Another sample weighing 5.00 g was found to contain 2.54 g of fluorine. The molar mass is found to be 448.4 g/mol. What are its empirical and molecular formulas? (AW(amu): C = 12.01, H = 1.008, F = 19.00)

The empirical and molecular formula of the compound is and  respectively

Explanation:

We are given:

Mass of

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 3.926 g of carbon dioxide, of carbon will be contained.

To calculate the percentage composition of element in sample, we use the equation:

     ......(1)

Mass of carbon = 1.071 g

Mass of sample = 2.50 g

Putting values in equation 1, we get:

Mass of fluorine = 2.54 g

Mass of sample = 5.00 g

Putting values in equation 1, we get:

Percent composition of hydrogen = [100 - 42.84 - 50.8] % = 6.36 %

We are given:

Percentage of C = 42.84 %

Percentage of F = 50.8 %

Percentage of H = 6.36 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of C = 42.84 g

Mass of F = 50.8 g

Mass of H = 6.36 g

To formulate the empirical formula, we need to follow some steps:

Moles of Carbon =

Moles of Hydrogen =

Moles of Fluorine =

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 2.67 moles.

For Carbon =

For Hydrogen =

For Fluorine =

The ratio of C : H : F = 1 : 2 : 1

The empirical formula for the given compound is

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

We are given:

Mass of molecular formula = 448.4 g/mol

Mass of empirical formula =

Putting values in above equation, we get:

Multiplying this valency by the subscript of every element of empirical formula, we get:

Hence, the empirical and molecular formula of the compound is and  respectively