A nitrogen and oxygen composiiof 4,6g contains 3,2g of oxygen
a) calculate the empirical formula of the compound
To calculate the empirical formula of the compound, we need to know the mass of nitrogen in the compound.
Given:
Mass of oxygen = 3.2g
Mass of nitrogen + Mass of oxygen = 4.6g
To find the mass of nitrogen, we can subtract the mass of oxygen from the total mass:
Mass of nitrogen = Total mass - Mass of oxygen
Mass of nitrogen = 4.6g - 3.2g
Mass of nitrogen = 1.4g
Now that we know the mass of nitrogen and oxygen, we can calculate the molar ratios of nitrogen to oxygen in the compound.
Moles of nitrogen = Mass of nitrogen / Molar mass of nitrogen
Molar mass of nitrogen = 14.01 g/mol (molar mass of nitrogen)
Moles of nitrogen = 1.4g / 14.01 g/mol = 0.0999 mol (rounded to 4 decimal places)
Moles of oxygen = Mass of oxygen / Molar mass of oxygen
Molar mass of oxygen = 16.00 g/mol (molar mass of oxygen)
Moles of oxygen = 3.2g / 16.00 g/mol = 0.2 mol
Now, let's divide the moles of each element by the smallest number of moles to get the empirical formula ratio:
Moles of nitrogen / 0.0999 mol = 0.0999 mol / 0.0999 mol = 1
Moles of oxygen / 0.0999 mol = 0.2 mol / 0.0999 mol = 2
So, the empirical formula of the compound is N1O2.
To calculate the empirical formula of the compound, we need to determine the ratio of nitrogen to oxygen atoms in the compound based on the given masses.
1. Convert the masses of nitrogen and oxygen to moles using their molar masses:
- Moles of nitrogen (N) = Mass of nitrogen (4.6 g) / Molar mass of nitrogen (14.01 g/mol).
- Moles of oxygen (O) = Mass of oxygen (3.2 g) / Molar mass of oxygen (16.00 g/mol).
2. Determine the simplest whole number ratio of nitrogen to oxygen by dividing both moles values by the smaller of the two:
- Divide the moles of each element by the smaller number of moles obtained.
3. Round the resulting ratio to the nearest whole number to obtain the empirical formula.
Let's calculate it step by step:
Moles of nitrogen (N) = 4.6 g / 14.01 g/mol ≈ 0.328 mol
Moles of oxygen (O) = 3.2 g / 16.00 g/mol = 0.200 mol
Since the smallest number of moles is 0.200 mol (oxygen), we can divide both moles by 0.200 mol:
Moles of nitrogen (N) ≈ 0.328 mol / 0.200 mol ≈ 1.64
Moles of oxygen (O) ≈ 0.200 mol / 0.200 mol = 1.00
Rounded to the nearest whole number, the ratio of nitrogen to oxygen is approximately 2:1.
Therefore, the empirical formula of the compound is N2O.