Question

111. При сгорании органического вещества массой 6,2 г получили 4,48 л углекислого газа (н.у.) и 5,4 г воды. Плотность паров вещества по азоту равна 2,214. Установите молекулярную формулу вещества.

Answer 1

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Answer 2

Calculation of the Molecular Formula

To determine the molecular formula of the substance, we need to analyze the given information about the combustion of the organic compound.

According to the information provided: - Mass of organic substance burned: 6.2 g - Volume of carbon dioxide produced (at standard temperature and pressure): 4.48 L - Mass of water produced: 5.4 g - Density of the vapor of the substance with respect to nitrogen: 2.214

To calculate the molecular formula, we need to find the number of moles of carbon dioxide and water produced.

1. Calculate the number of moles of carbon dioxide: - The molar volume of any gas at standard temperature and pressure (STP) is 22.4 L. - Using the molar volume, we can calculate the number of moles of carbon dioxide produced: ``` Moles of CO2 = Volume of CO2 / Molar volume of CO2 at STP = 4.48 L / 22.4 L/mol = 0.2 mol ```

2. Calculate the number of moles of water: - The molar mass of water (H2O) is 18 g/mol. - Using the molar mass, we can calculate the number of moles of water produced: ``` Moles of H2O = Mass of H2O / Molar mass of H2O = 5.4 g / 18 g/mol = 0.3 mol ```

3. Determine the empirical formula: - The empirical formula represents the simplest whole-number ratio of atoms in a compound. - To find the empirical formula, we need to determine the ratio of carbon to hydrogen in the compound. - From the balanced equation for the combustion of organic compounds, we know that for every 1 mole of carbon dioxide produced, there are 1 mole of carbon atoms. - Similarly, for every 1 mole of water produced, there are 2 moles of hydrogen atoms. - Therefore, the empirical formula is CH2O.

4. Determine the molecular formula: - The molecular formula represents the actual number of atoms of each element in a compound. - To find the molecular formula, we need to know the molar mass of the compound. - The molar mass of the empirical formula CH2O is: ``` Molar mass of CH2O = (12.01 g/mol) + (2 * 1.01 g/mol) + (16.00 g/mol) = 30.03 g/mol ```

- To calculate the ratio of the molar mass of the compound to the molar mass of the empirical formula, we divide the molar mass of the compound by the molar mass of the empirical formula: ``` Ratio = Molar mass of compound / Molar mass of empirical formula = 6.2 g / 30.03 g/mol = 0.206 mol ```

- The ratio of 0.206 mol indicates that the molecular formula is approximately one-fifth of the empirical formula. - Therefore, the molecular formula of the substance is approximately C5H10O2.

Please note that the given information does not provide enough data to determine the exact molecular formula. The calculation assumes that the substance is a simple organic compound and follows the principles of stoichiometry.