Question

при сгорании углеводорода массой 10,32 г, плотность паров по водороду которого равна 43, образовался углекислый газ объемом 16,128 л (н.у.) и вода массой 15,12 г. Выведите молекулярную формулу углеводорода, составьте формулы изомеров, соответствующих этой формуле, и дайте им названия

Answer 1

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Answer 2

Calculation of Molecular Formula

To determine the molecular formula of the hydrocarbon, we need to analyze the given information about the mass, density of the vapor, and the volume of carbon dioxide and water produced during combustion.

Given: - Mass of hydrocarbon = 10.32 g - Density of vapor (relative to hydrogen) = 43 - Volume of carbon dioxide produced = 16.128 L (at standard temperature and pressure) - Mass of water produced = 15.12 g

To find the molecular formula, we can follow these steps:

Step 1: Calculate the number of moles of carbon dioxide produced. - The volume of carbon dioxide is given at standard temperature and pressure (STP), which is 1 mole of any gas at 22.4 L. - Using the volume of carbon dioxide produced (16.128 L), we can calculate the number of moles of carbon dioxide produced.

Step 2: Calculate the number of moles of water produced. - The molar mass of water (H2O) is 18 g/mol. - Using the mass of water produced (15.12 g), we can calculate the number of moles of water produced.

Step 3: Calculate the number of moles of carbon and hydrogen in the hydrocarbon. - Since the hydrocarbon only contains carbon and hydrogen, we can assume that all the carbon in the hydrocarbon is converted to carbon dioxide and all the hydrogen is converted to water during combustion. - From the number of moles of carbon dioxide and water produced, we can calculate the number of moles of carbon and hydrogen in the hydrocarbon.

Step 4: Determine the empirical formula. - Divide the number of moles of carbon and hydrogen by the smallest number of moles obtained. - This will give us the empirical formula of the hydrocarbon.

Step 5: Determine the molecular formula. - The empirical formula gives us the simplest ratio of atoms in the hydrocarbon. - To find the molecular formula, we need to know the molar mass of the hydrocarbon. - We can calculate the molar mass by adding up the atomic masses of the elements in the empirical formula. - Divide the molar mass of the hydrocarbon by the molar mass of the empirical formula to find the number of empirical formula units in the molecular formula.

Let's perform the calculations:

Step 1: Calculate the number of moles of carbon dioxide produced. - The volume of carbon dioxide produced is 16.128 L. - At STP, 1 mole of any gas occupies 22.4 L. - Therefore, the number of moles of carbon dioxide produced is 16.128 L / 22.4 L/mol = 0.721 mole.

Step 2: Calculate the number of moles of water produced. - The molar mass of water (H2O) is 18 g/mol. - The mass of water produced is 15.12 g. - Therefore, the number of moles of water produced is 15.12 g / 18 g/mol = 0.84 mole.

Step 3: Calculate the number of moles of carbon and hydrogen in the hydrocarbon. - Since the hydrocarbon only contains carbon and hydrogen, we can assume that all the carbon in the hydrocarbon is converted to carbon dioxide and all the hydrogen is converted to water during combustion. - From the number of moles of carbon dioxide and water produced, we can calculate the number of moles of carbon and hydrogen in the hydrocarbon. - From the balanced chemical equation for the combustion of hydrocarbons, we know that 1 mole of carbon dioxide is produced for every 1 mole of carbon in the hydrocarbon, and 1 mole of water is produced for every 2 moles of hydrogen in the hydrocarbon. - Therefore, the number of moles of carbon in the hydrocarbon is 0.721 mole, and the number of moles of hydrogen in the hydrocarbon is 2 * 0.84 mole = 1.68 mole.

Step 4: Determine the empirical formula. - Divide the number of moles of carbon and hydrogen by the smallest number of moles obtained. - The smallest number of moles obtained is 0.721 mole. - Therefore, the empirical formula of the hydrocarbon is C0.721H1.68.

Step 5: Determine the molecular formula. - To find the molecular formula, we need to know the molar mass of the hydrocarbon. - We can calculate the molar mass by adding up the atomic masses of the elements in the empirical formula. - The atomic mass of carbon (C) is 12 g/mol, and the atomic mass of hydrogen (H) is 1 g/mol. - The molar mass of the empirical formula C0.721H1.68 is (0.721 * 12 g/mol) + (1.68 * 1 g/mol) = 8.652 g/mol + 1.68 g/mol = 10.332 g/mol.

- Divide the molar mass of the hydrocarbon (10.32 g) by the molar mass of the empirical formula (10.332 g/mol) to find the number of empirical formula units in the molecular formula. - The molecular formula of the hydrocarbon is therefore C0.721H1.68 * (10.32 g / 10.332 g/mol) = C0.721H1.68.

Isomers and Names

The molecular formula of the hydrocarbon is C0.721H1.68.

Isomers are compounds that have the same molecular formula but different structural arrangements. To determine the isomers corresponding to this molecular formula, we need more information about the connectivity of the atoms in the hydrocarbon.

Without additional information about the connectivity of the atoms, it is not possible to determine the specific isomers corresponding to the molecular formula C0.721H1.68.

Therefore, we cannot provide the specific isomers or their names without additional information.

Please provide more details about the connectivity of the atoms in the hydrocarbon to determine the specific isomers and their names.