Question

Азотосодержащее органическое соединение массой 11,8 г,плотность паров которого по воздуху равна 2,035,сожгли в избытке кислорода.При этом образовался оксид углерода(IV)объемом 13,44 л,азот объемом 2,2411(н.у) и вода массой 16,2 г.Выделите молекулярную формулу этого вещества

Answer 1

N(co2)=13,44/22,4=0,6
n(c)=0,6
n(n2)=0,1
n(N)=0,1*2=0,2
n(h2o)=16,2/18=0,9
n(h)=2*0,9=1,8
0,6:1,8:0,2=3:9:1
C3H9N

Answer 2

Molecular Formula of the Organic Compound

To determine the molecular formula of the organic compound described, we need to analyze the information provided.

The mass of the organic compound is given as 11.8 g, and its vapor density with respect to air is 2.035. Additionally, when the compound was burned in excess oxygen, it produced carbon dioxide with a volume of 13.44 L, nitrogen with a volume of 2.2411 (at normal conditions), and water with a mass of 16.2 g.

To find the molecular formula, we can start by calculating the molar mass of the compound. The molar mass is the mass of one mole of a substance and is expressed in grams per mole (g/mol).

Using the given information, we can calculate the molar mass of the organic compound as follows:

1. Calculate the moles of carbon dioxide produced: - The volume of carbon dioxide produced is 13.44 L. - At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 L. - Therefore, the moles of carbon dioxide produced can be calculated as: 13.44 L / 22.4 L/mol = 0.6 mol.

2. Calculate the moles of nitrogen produced: - The volume of nitrogen produced is 2.2411 (at normal conditions). - Therefore, the moles of nitrogen produced can be calculated as: 2.2411 mol.

3. Calculate the moles of water produced: - The mass of water produced is 16.2 g. - The molar mass of water (H2O) is approximately 18 g/mol. - Therefore, the moles of water produced can be calculated as: 16.2 g / 18 g/mol = 0.9 mol.

4. Calculate the moles of carbon and hydrogen in the organic compound: - The moles of carbon can be calculated by multiplying the moles of carbon dioxide produced by the ratio of carbon atoms in carbon dioxide (1 carbon atom per 1 molecule of carbon dioxide). - The moles of carbon can be calculated as: 0.6 mol. - The moles of hydrogen can be calculated by multiplying the moles of water produced by the ratio of hydrogen atoms in water (2 hydrogen atoms per 1 molecule of water). - The moles of hydrogen can be calculated as: 1.8 mol.

5. Calculate the moles of nitrogen in the organic compound: - The moles of nitrogen can be calculated as: 2.2411 mol.

6. Calculate the total moles of the organic compound: - The total moles of the organic compound can be calculated by summing the moles of carbon, hydrogen, and nitrogen: - Total moles = moles of carbon + moles of hydrogen + moles of nitrogen - Total moles = 0.6 mol + 1.8 mol + 2.2411 mol = 4.6411 mol.

Now that we have the total moles of the organic compound, we can calculate its molar mass by dividing the mass of the compound by the total moles:

Molar mass = mass of the compound / total moles Molar mass = 11.8 g / 4.6411 mol ≈ 2.54 g/mol

The molar mass of the organic compound is approximately 2.54 g/mol.

Unfortunately, the search results did not provide the molecular formula of the organic compound directly. However, with the molar mass of approximately 2.54 g/mol, further analysis and experimentation would be required to determine the specific molecular formula of the compound.