Deduce the number of nitrogen atoms in:
5.00 x 10^-3 mol of ammonia, NH3
and
4.601 g of nitrogen dioxide, NO2
There are 6.02E23 molecules in 1 mol.
In 5.00E-3 mols NH3 there are 5.00E-3 x 6.02E23 molecules = approx 3E21.
Then there is 1 N atom in 1 molecule of NH3; therefore, there must be about 3E21 atoms N. If your prof is picky about significant figures you need to make the answer consistent with those rules.
The second one is done the same way.
So, you don't have to do anything about the H3 or the O2?
Yes and no. First, the problem asks about N and not H. You do use H in determining the molar mass NH3 which is 14 for N and 3*1 = 3 for H to make 17 for NH3. Since you know the number of atoms of N, however, it is easy to calculate the number of atoms of H in NH3. It's just 3x that.
Thank you for the help!
Sure, let me calculate that for you... Just converting some units into clown language. 🤡
For 5.00 x 10^-3 mol of ammonia, NH3, we can use Avogadro's number to find the number of nitrogen atoms. Since ammonia has only one nitrogen atom, we can say that there are:
5.00 x 10^-3 moles of NH3 × 6.022 x 10^23 🤡 nitrogen atoms/mole of NH3 = 3.011 x 10^21 🤡 nitrogen atoms in 5.00 x 10^-3 mol of ammonia.
Now, let's move on to nitrogen dioxide, NO2. To find the number of nitrogen atoms in 4.601 g, we need to know the molar mass of NO2. Nitrogen has a molar mass of around 14 g/mol, and since NO2 has one nitrogen atom, we can calculate it like this:
4.601 g ÷ 46 g/mol = 0.1 mol of NO2
Since NO2 has one nitrogen atom, we can say that there are:
0.1 moles of NO2 × 6.022 x 10^23 🤡 nitrogen atoms/mole of NO2 = 6.022 x 10^22 🤡 nitrogen atoms in 4.601 g of nitrogen dioxide.
So, there you have it! Approximately 3.011 x 10^21 🤡 nitrogen atoms in 5.00 x 10^-3 mol of ammonia, and approximately 6.022 x 10^22 🤡 nitrogen atoms in 4.601 g of nitrogen dioxide. Hope that helps! 🤡
To deduce the number of nitrogen atoms in a given sample, we need to use Avogadro's number, which is approximately 6.022 x 10^23 particles per mole.
1) For 5.00 x 10^-3 mol of ammonia, NH3:
Since ammonia has one nitrogen atom per molecule, we can directly calculate the number of nitrogen atoms using Avogadro's number.
Number of nitrogen atoms = (Number of moles) x (Avogadro's number)
= (5.00 x 10^-3 mol) x (6.022 x 10^23 particles/mol)
≈ 3.011 x 10^20 nitrogen atoms
Therefore, there are approximately 3.011 x 10^20 nitrogen atoms in 5.00 x 10^-3 mol of ammonia.
2) For 4.601 g of nitrogen dioxide, NO2:
To calculate the number of nitrogen atoms, we first need to determine the number of moles of nitrogen dioxide.
Number of moles = (Mass of substance) / (Molar mass)
The molar mass of nitrogen dioxide (NO2) is:
Molar mass of NO2 = (Atomic mass of nitrogen) + 2 x (Atomic mass of oxygen)
= (14.01 g/mol) + 2 x (16.00 g/mol)
= 46.01 g/mol
Now we can calculate the number of moles of nitrogen dioxide:
Number of moles = (Mass of substance) / (Molar mass)
= (4.601 g) / (46.01 g/mol)
≈ 0.100 mol
Since nitrogen dioxide has one nitrogen atom per molecule, the number of nitrogen atoms is simply equal to the number of moles.
Number of nitrogen atoms ≈ 0.100 mol
Therefore, there are approximately 0.100 moles (which is equivalent to 0.100 x 6.022 x 10^23) of nitrogen atoms in 4.601 g of nitrogen dioxide.