<u>Answer:</u> The empirical formula for the given organic compound is 
<u>Explanation:</u>
The chemical equation for the combustion of hydrocarbon having carbon and hydrogen follows:

where, 'x' and 'y' are the subscripts of Carbon and hydrogen respectively.
We are given:
Mass of
(Conversion factor: 1 g = 1000 mg)
Mass of 
We know that:
Molar mass of carbon dioxide = 44 g/mol
Molar mass of water = 18 g/mol
- <u>For calculating the mass of carbon:</u>
In 44g of carbon dioxide, 12 g of carbon is contained.
So, in
of carbon dioxide,
of carbon will be contained.
- <u>For calculating the mass of hydrogen:</u>
In 18g of water, 2 g of hydrogen is contained.
So, in
of water,
of hydrogen will be contained.
To formulate the empirical formula, we need to follow some steps:
- <u>Step 1:</u> Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen = 
- <u>Step 2:</u> Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 
For Carbon = 
For Hydrogen = 
- <u>Step 3:</u> Taking the mole ratio as their subscripts.
The ratio of C : H = 1 : 1
Hence, the empirical formula for the given compound is 