Question

Определить молекулярную формулу соединения, если массовая доля серы – 94%, массовая доля водорода 6%, относительная молекулярная масса соединения 34.

Answer 1

Н    S
6 /1    94/32
6/3   3/3
2      1
Н 2S   М=34

Answer 2

Molecular Formula Calculation

To determine the molecular formula of the compound with a sulfur mass fraction of 94%, a hydrogen mass fraction of 6%, and a relative molecular mass of 34, we can follow these steps:

Step 1: Convert the mass fractions to moles. - The mass fraction of sulfur is 94%, which means that for every 100 grams of the compound, 94 grams are sulfur. - The mass fraction of hydrogen is 6%, which means that for every 100 grams of the compound, 6 grams are hydrogen.

To convert these mass fractions to moles, we need to know the molar masses of sulfur and hydrogen.

According to source the molar mass of sulfur (S) is approximately 32.06 g/mol, and the molar mass of hydrogen (H) is approximately 1.01 g/mol.

Using these molar masses, we can calculate the number of moles of sulfur and hydrogen in 100 grams of the compound:

- Moles of sulfur = (mass of sulfur / molar mass of sulfur) = (94 g / 32.06 g/mol) - Moles of hydrogen = (mass of hydrogen / molar mass of hydrogen) = (6 g / 1.01 g/mol)

Step 2: Determine the empirical formula. - The empirical formula represents the simplest whole number ratio of atoms in a compound. - To find the empirical formula, we divide the number of moles of each element by the smallest number of moles obtained.

Let's calculate the number of moles of sulfur and hydrogen:

- Moles of sulfur = (94 g / 32.06 g/mol) ≈ 2.93 mol - Moles of hydrogen = (6 g / 1.01 g/mol) ≈ 5.94 mol

The smallest number of moles obtained is approximately 2.93 mol, which corresponds to sulfur. Therefore, the empirical formula will have a ratio of approximately 2.93 moles of sulfur to 2.93 moles of hydrogen.

Step 3: 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 relative molecular mass of the compound.

According to the given information, the relative molecular mass of the compound is 34.

To calculate the molecular formula, we divide the relative molecular mass by the empirical formula mass and multiply the subscripts in the empirical formula by this factor.

The empirical formula mass can be calculated by summing the molar masses of the atoms in the empirical formula.

The molar mass of sulfur is approximately 32.06 g/mol, and the molar mass of hydrogen is approximately 1.01 g/mol.

The empirical formula mass is approximately (2.93 mol * 32.06 g/mol) + (2.93 mol * 1.01 g/mol).

Let's calculate the empirical formula mass:

- Empirical formula mass ≈ (2.93 mol * 32.06 g/mol) + (2.93 mol * 1.01 g/mol) ≈ 94.01 g/mol

Now, we can calculate the factor to determine the molecular formula:

- Factor = (relative molecular mass) / (empirical formula mass) = 34 / 94.01 ≈ 0.361

Finally, we multiply the subscripts in the empirical formula by the factor to obtain the molecular formula:

- Molecular formula = (empirical formula) * (factor)

Based on the calculations, the molecular formula of the compound is approximately S1H2.

Please note that the given information and calculations are approximate and may not represent the exact molecular formula of the compound.