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The following diagram represents the collection of CO2 and H2O molecules formed by complete combustion of a hydrocarbon. (Figure 1)

What is the empirical formula of the hydrocarbon?
Express your answer as a chemical formula.

The following diagram represents the collection of CO2 and H2O molecules formed by complete combustion of a hydrocarbon Figure 1 What is the empirical formula o class=

Respuesta :

Answer: [tex]CH_4[/tex] is the empirical formula of the hydrocarbon.

Explanation: Combustion reactions are the one where hydrocarbon in the presence of oxygen decomposes to carbon dioxide and water molecule.

General equation for combustion reaction:

[tex]Hydrocarbon+O_2\rightarrow CO_2+H_2O[/tex]

In the image, the molecule having red and black balls are carbon dioxide and the molecules having red and white balls are water molecules.

Moles of Carbon dioxide molecule are 4 which means that the there are 4 moles of carbon and 8 moles of oxygen atoms.

Moles of water molecules are 8 which means that there are 16 moles of hydrogen and 8 moles of oxygen atoms.

Thus, According to the law of conservation of mass, there should be same number of moles of each element on the reactant side as well, which gives us the molecular formula of the hydrocarbon as [tex]C_4H_{16}[/tex]

Empirical formula is the one in which the elements in a molecule are in simplest whole number ratio. Hence, the empirical formula becomes [tex]CH_4[/tex].

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The empirical formula of the hydrocarbon is [tex]\rm CH_4[/tex]

What are combustion reaction?

Combustion reactions are those in which the substance react with oxygen and produce heat and light.

In the given case, the red and black compound is carbon dioxide and the red and white compound are oxygen.

There are 4 moles of carbon dioxide and 8 moles of oxygen are present.

On the complete combustion of methane, we will get carbon dioxide and oxygen molecules.

Thus, the empirical formula is [tex]\rm CH_4[/tex]

Learn more about combustion reaction, here

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Thus, According to the law of conservation of mass, there should be same number of moles of each element on the reactant side as well, which gives us the molecular formula of the hydrocarbon as

Empirical formula is the one in which the elements in a molecule are in simplest whole number ratio. Hence, the empirical formula becomes

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