A gaseous organic compound containing only carbon, hydrogen, and nitrogen is burned in oxygen gas, and the volume of each reactant and product is measured under the same conditions of temperature and pressure. Reaction of four volumes of the compound produces four volumes of CO₂, two volumes of N₂, and ten volumes of water vapor. (b) What is the empirical formula of the compound?

Let the compound will be [tex]C_{x} H_{y} N_{z}[/tex] and combustion of this molecule in presence of oxygen gives carbon dioxide , nitrogen and water molecule as ,

[tex]C_{x} H_{y} N_{z}[/tex] + [tex]O_{2}[/tex] → [tex]N_{2}[/tex] + [tex]CO_{2}[/tex] + [tex]H_{2} O[/tex]

4 vol 2 vol 4 vol 10 vol

The equation will be as

4[tex]C_{x} H_{y} N_{z}[/tex] + [tex]O_{2}[/tex] → 2[tex]N_{2}[/tex] + 4[tex]CO_{2}[/tex] + 10[tex]H_{2} O[/tex]

Number of carbon atom in right side = 4

Number of carbon atom in left hand = 4

So value of x = 1

Number of hydrogen atom in right side = 4

Number of hydrogen atom in left side = 20

So value of y = 5

Number of nitrogen atom in right side = 4

Number of nitrogen atom in left side = 4

So value of y = 1

So the molecular formula of [tex]C_{x} H_{y} N_{z}[/tex] is [tex]C_{} H_{5} N_{}[/tex] or [tex]C_{} H_{3} NH_{2}[/tex]

The empirical formula of the compound = [tex]C_{} H_{3} NH_{2}[/tex]

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