Question

Пожалуйста, помогите! 100 балов! 1)Внаслідок спалювання 13,8 г речовини добули вуглекислий газ обемом 23,52 л та 0,5 моль водн. Відносна густина пари речовини за воднем дорівнює 46. Знайдіть молекулярну формулу речовини. 2)Органічна речовина має відносну густину пари за воднем 46. Зразок цієї речовини масою 13,8 Г спалили, Дiставши оксид карбону (IV) об'ємом 23,52 л (нормальні умови) та воду масою 10,8 г. Визначте формулу органічної речовини, враховуючи, що вона ароматична ​

Answer 1

Объяснение:

Это если что была домашка поэтому вот и сделай пожалуйста лучшим ответом!!!!

Просто тот ответ до сих пор не сделал(а) если не сделаешь я удалю сразу,сделай пж сразу!!!

Answer 2

Finding the Molecular Formula of a Substance

To find the molecular formula of a substance, we need to analyze the given information and use the principles of stoichiometry and the ideal gas law.

1) In this case, we are given that 13.8 g of a substance was burned, producing 23.52 L of carbon dioxide gas (CO2) and 0.5 moles of hydrogen gas (H2). The relative density of the substance's vapor to hydrogen is 46.

To find the molecular formula, we can follow these steps: - Calculate the number of moles of carbon dioxide gas produced using its molar mass. - Calculate the number of moles of hydrogen gas produced. - Determine the empirical formula of the substance by dividing the number of moles of each element by the smallest number of moles obtained. - Calculate the molecular formula using the empirical formula and the relative density of the substance's vapor to hydrogen.

Let's calculate the values step by step:

- The molar mass of carbon dioxide (CO2) is 44.01 g/mol. Using this, we can calculate the number of moles of carbon dioxide gas produced: - Moles of CO2 = mass of CO2 / molar mass of CO2 - Moles of CO2 = 23.52 L * (1 mol / 22.4 L) = 1.05 mol

- The number of moles of hydrogen gas produced is given as 0.5 mol.

- Now, let's determine the empirical formula of the substance: - Divide the number of moles of each element by the smallest number of moles obtained. - The smallest number of moles obtained is 0.5 mol, which corresponds to hydrogen. - Moles of carbon = 1.05 mol / 0.5 mol = 2.1 mol

- The empirical formula of the substance is H2C2O4.

- Finally, we can calculate the molecular formula using the empirical formula and the relative density of the substance's vapor to hydrogen: - The relative density of the substance's vapor to hydrogen is 46. - The molar mass of the empirical formula H2C2O4 is 90.04 g/mol. - The molecular formula can be calculated by multiplying the empirical formula by a factor of n: - Molecular formula = (H2C2O4)n - n = (molar mass of molecular formula) / (molar mass of empirical formula) - n = 46 / 90.04 ≈ 0.51

- The molecular formula is approximately H1C1O2.

Therefore, the molecular formula of the substance is HC2O4.

2) In this case, we are given that 13.8 g of an organic substance was burned, producing 23.52 L of carbon dioxide gas (CO2) and 10.8 g of water (H2O). The relative density of the substance's vapor to hydrogen is 46, and it is mentioned that the substance is aromatic.

Using the same steps as above, we can calculate the molecular formula of the organic substance:

- Calculate the number of moles of carbon dioxide gas produced using its molar mass. - Calculate the number of moles of water produced using its molar mass. - Determine the empirical formula of the substance by dividing the number of moles of each element by the smallest number of moles obtained. - Calculate the molecular formula using the empirical formula and the relative density of the substance's vapor to hydrogen.

Let's calculate the values step by step:

- The molar mass of carbon dioxide (CO2) is 44.01 g/mol. Using this, we can calculate the number of moles of carbon dioxide gas produced: - Moles of CO2 = mass of CO2 / molar mass of CO2 - Moles of CO2 = 23.52 L * (1 mol / 22.4 L) = 1.05 mol

- The molar mass of water (H2O) is 18.02 g/mol. Using this, we can calculate the number of moles of water produced: - Moles of H2O = mass of H2O / molar mass of H2O - Moles of H2O = 10.8 g / 18.02 g/mol ≈ 0.6 mol

- Now, let's determine the empirical formula of the substance: - Divide the number of moles of each element by the smallest number of moles obtained. - The smallest number of moles obtained is 0.6 mol, which corresponds to water. - Moles of carbon = 1.05 mol / 0.6 mol ≈ 1.75 mol

- The empirical formula of the substance is H2C1.75O1.

- Finally, we can calculate the molecular formula using the empirical formula and the relative density of the substance's vapor to hydrogen: - The relative density of the substance's vapor to hydrogen is 46. - The molar mass of the empirical formula H2C1.75O1 is approximately 59.8 g/mol. - The molecular formula can be calculated by multiplying the empirical formula by a factor of n: - Molecular formula = (H2C1.75O1)n - n = (molar mass of molecular formula) / (molar mass of empirical formula) - n = 46 / 59.8 ≈ 0.77

- The molecular formula is approximately H1.54C1.35O1.

Therefore, the molecular formula of the organic substance is approximately H1.54C1.35O1.