The empirical formula of an oxide of nitrogen containg 30.4 per cent of nitrogen is NO
To determine the empirical formula of the oxide of nitrogen, we need to know the percentages of each element present. In this case, we are given that the oxide contains 30.4% nitrogen.
To find the empirical formula, we can assume a 100-gram sample of the compound. This means that 30.4 grams of the sample will be nitrogen.
To find the amount of oxygen, we subtract the nitrogen's mass from the total mass of the sample:
Total mass of the sample = 100 grams
Mass of nitrogen = 30.4 grams
Mass of oxygen = Total mass - Mass of nitrogen = 100 grams - 30.4 grams = 69.6 grams
Now that we know the masses of nitrogen and oxygen, we need to convert them into moles. The molar mass of nitrogen (N) is 14.01 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol.
Number of moles of nitrogen = Mass of nitrogen / Molar mass of nitrogen = 30.4 grams / 14.01 g/mol ≈ 2.17 moles
Number of moles of oxygen = Mass of oxygen / Molar mass of oxygen = 69.6 grams / 16.00 g/mol ≈ 4.35 moles
Next, we need to find the ratio of nitrogen to oxygen by dividing the number of moles of each element by the smallest number of moles:
Nitrogen: Oxygen ≈ 2.17 moles: 4.35 moles
Dividing both moles by the smallest number (2.17), we get:
Nitrogen: Oxygen ≈ 1 mole: 2 moles
Finally, we can write the empirical formula using the ratio of nitrogen to oxygen:
Empirical formula = NO2
Therefore, the empirical formula of the oxide of nitrogen containing 30.4% nitrogen is NO2.
To determine the empirical formula of an oxide of nitrogen containing 30.4% of nitrogen, we need to use the concept of empirical formula calculations. Here's the step-by-step process:
1. Assume we have a 100g sample of the oxide.
2. From the given percentage, we know that the oxide contains 30.4g of nitrogen.
3. To find the amount of oxygen, subtract the nitrogen weight from the total sample weight. In this case, 100g - 30.4g = 69.6g of oxygen.
4. Next, we need to convert the masses of nitrogen and oxygen into moles by dividing each by their respective molar masses.
- The molar mass of nitrogen (N) is 14g/mol.
- The molar mass of oxygen (O) is 16g/mol.
- For nitrogen: 30.4g / 14g/mol = 2.17 mol of nitrogen.
- For oxygen: 69.6g / 16g/mol = 4.35 mol of oxygen.
5. Divide the number of moles of each element by the smallest one to find the simplest whole number ratio of elements in the compound.
- Nitrogen: 2.17 mol / 2.17 mol = 1 (rounded to the nearest whole number).
- Oxygen: 4.35 mol / 2.17 mol ≈ 2 (rounded to the nearest whole number).
6. Finally, write the empirical formula using the whole number ratios obtained in the previous step. The empirical formula of the oxide of nitrogen is NO.
In conclusion, the empirical formula of the nitrogen oxide with 30.4% nitrogen composition is NO.