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. Dimethyl nitrosamine is a known carcinogen. It can be formed in the intestinal tract when digestive juices react with the nitrite ion is preserved and smoked meats. It is made up of carbon, hydrogen, nitrogen, and oxygen atoms. A 4.319 g sample of dimethyl nitrosamine burned in oxygen yields 5.134 g of CO2 and 3.173 g of H2 O. The compound contains 37,82% by mass of nitrogen. What is the empirical formula of dimethyl nitrosamine?

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Answer: The empirical formula for the given compound is
C_2H_6ON_2

Step-by-step explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:


C_xH_yN_z+O_2\rightarrow CO_2+H_2O

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and nitrogen respectively.

We are given:

Mass of
CO_2=5.134g

Mass of
H_2O=3.173g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

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

So, in 5.134 g of carbon dioxide,
(12)/(44)* 5.134=1.4g of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 3.173 g of water,
(2)/(18)* 3.173=0.35g of hydrogen will be contained.

For calculating the mass of nitrogen:

As, 100 g of sample contains 37.87 % of nitrogen

So, 4.319 g of sample contains
(37.87)/(100)* 4.319=1.635g of nitrogen

For calculating the mass of oxygen:

Mass of oxygen in the compound = (4.319) - (1.4 + 0.35 + 1.635) = 0.934 g

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

Step 1: Converting the given masses into moles.

Moles of Carbon =
\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=(1.4g)/(12g/mole)=0.116moles

Moles of Hydrogen =
\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=(0.35g)/(1g/mole)=0.35moles

Moles of Oxygen =
\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=(0.934g)/(16g/mole)=0.058moles

Moles of Nitrogen =
\frac{\text{Given mass of nitrogen}}{\text{Molar mass of nitrogen}}=(1.635g)/(14g/mole)=0.116moles

Step 2: 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 0.058 moles.

For Carbon =
(0.116)/(0.058)=2

For Hydrogen =
(0.35)/(0.058)=6.03\approx 6

For Oxygen =
(0.058)/(0.058)=1

For Oxygen =
(0.116)/(0.058)=2

Step 3: Taking the mole ratio as their subscripts.

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

Hence, the empirical formula for the given compound is
C_2H_6O_1N_2=C_2H_6ON_2

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