Question

При сгорании углеводорода образовалось 22 г оксида углерода(IV) и 10,8 г воды. Относительная плотность этого вещества по водороду равна 36. Определите молекулярную формулу этого вещества. HELP

Answer 1

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Answer 2

Calculation of Molecular Formula

To determine the molecular formula of the substance formed during the combustion of hydrocarbon, we need to analyze the given information.

Given: - Mass of carbon dioxide (CO2) formed = 22 g - Mass of water (H2O) formed = 10.8 g - Relative density of the substance with respect to hydrogen = 36

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

1. Calculate the number of moles of carbon dioxide (CO2): - The molar mass of carbon dioxide (CO2) is 44 g/mol (12 g/mol for carbon + 2 * 16 g/mol for oxygen). - Number of moles of CO2 = Mass of CO2 / Molar mass of CO2 = 22 g / 44 g/mol = 0.5 mol

2. Calculate the number of moles of water (H2O): - The molar mass of water (H2O) is 18 g/mol (2 * 1 g/mol for hydrogen + 16 g/mol for oxygen). - Number of moles of H2O = Mass of H2O / Molar mass of H2O = 10.8 g / 18 g/mol = 0.6 mol

Now, let's analyze the ratio of carbon dioxide to water formed during the combustion.

- The ratio of moles of carbon dioxide to water is 0.5 mol : 0.6 mol, which simplifies to 5 : 6.

To find the empirical formula, we divide the subscripts by their greatest common divisor (GCD), which is 1 in this case.

- The empirical formula is therefore C5H6.

Next, we need to determine the molecular formula by finding the ratio between the empirical formula and the molecular formula.

- The relative density of the substance with respect to hydrogen is given as 36. This means that the molecular formula is 36 times the empirical formula.

- The molecular formula is therefore (C5H6)36, which simplifies to C180H216.

Please note that the given information does not provide the specific hydrocarbon or its molecular formula. The calculation above is based solely on the given masses of carbon dioxide and water formed during the combustion and the relative density of the substance with respect to hydrogen.