Determine the empirical formula for a compound that contains c, h and o. it contains 52.14% c and 34.73% o by mass. what is the molecular formula if the molar mass is 92 g/mol?

The molecular formula for the given organic compound is

Explanation:

We are given:

Percentage of C = 52.14 %

Percentage of O = 34.73 %

Percentage of H = (100 - 52.14 - 34.73) = 13.13 %

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

Mass of C = 52.14 g

Mass of O = 34.73 g

Mass of H = 13.13 g

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

Moles of Carbon =

Moles of Oxygen =

Moles of Hydrogen =

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 2.171 moles.

For Carbon =

For Oxygen =

For Hydrogen =

The ratio of C : O : H = 2 : 1 : 6

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 = 92 g/mol

Mass of empirical formula = 46 g/mol

Putting values in above equation, we get:

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

Hence, the molecular formula for the given organic compound is

fe 55.85 g/mol and h2o 18.02 g/mol.