Question

Срочно.!!Определите молекулярную формулу соединения, содержащего 87,5% азота и 12,5% водорода, если его плотность по водороду равна 16. желательно с решением и формулами!!

Answer 1

Думаю,что так......................

Answer 2

Molecular Formula Calculation

To determine the molecular formula of the compound containing 87.5% nitrogen and 12.5% hydrogen, we can follow these steps:

1. Assume we have 100 grams of the compound. 2. Calculate the number of moles of nitrogen and hydrogen in the compound. 3. Determine the simplest ratio of nitrogen to hydrogen. 4. Find the empirical formula of the compound. 5. Calculate the molar mass of the empirical formula. 6. Determine the molecular formula using the molar mass and the empirical formula.

Let's go through each step in detail:

Step 1: Assume 100 grams of the compound

Assuming we have 100 grams of the compound, we have 87.5 grams of nitrogen and 12.5 grams of hydrogen.

Step 2: Calculate the number of moles of nitrogen and hydrogen

To calculate the number of moles, we need to divide the mass of each element by its molar mass.

The molar mass of nitrogen (N) is approximately 14.01 g/mol, and the molar mass of hydrogen (H) is approximately 1.01 g/mol.

Number of moles of nitrogen = 87.5 g / 14.01 g/mol = 6.24 mol Number of moles of hydrogen = 12.5 g / 1.01 g/mol = 12.38 mol

Step 3: Determine the simplest ratio of nitrogen to hydrogen

To find the simplest ratio, we need to divide the number of moles of each element by the smallest number of moles.

Dividing both moles of nitrogen and hydrogen by 6.24 (the smallest number of moles), we get:

Number of moles of nitrogen = 6.24 mol / 6.24 mol = 1 mol Number of moles of hydrogen = 12.38 mol / 6.24 mol = 1.98 mol

The simplest ratio is 1:1, which means the empirical formula will have one nitrogen atom and one hydrogen atom.

Step 4: Find the empirical formula of the compound

The empirical formula represents the simplest whole-number ratio of atoms in a compound. In this case, the empirical formula is NH.

Step 5: Calculate the molar mass of the empirical formula

The molar mass of the empirical formula NH can be calculated by summing the molar masses of nitrogen and hydrogen:

Molar mass of NH = (1 mol of N) * (14.01 g/mol) + (1 mol of H) * (1.01 g/mol) = 15.02 g/mol

Step 6: Determine the molecular formula using the molar mass and the empirical 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.

Given that the density of the compound with respect to hydrogen is 16, we can calculate the molar mass of the compound.

Molar mass of the compound = 16 g/mol

To find the molecular formula, we divide the molar mass of the compound by the molar mass of the empirical formula:

Molar mass of the compound / Molar mass of the empirical formula = 16 g/mol / 15.02 g/mol ≈ 1.066

Since the result is close to 1, the molecular formula is the same as the empirical formula.

Therefore, the molecular formula of the compound is NH.

Please note that the given search results did not provide specific information related to the question. The calculation and explanation provided above are based on general knowledge of chemistry and the principles of empirical and molecular formulas.