Answer:
1.14×10²³ atoms of N are contained in 4.19 g of N₂O
Explanation:
Nitrous oxide → N₂O
You must begin with this rule.
1 mol of compound has x moles of each element, for example:
1 mol of water has 2 moles of H and 1 mol of O (H₂O)
1 mol of ammonia has 3 moles of H and 1 mol of N (NH₃)
Then, 1 mol of N₂O has 2 moles of oxygen and 1 mol of O
The molar mass for our compound is 44 g/mol
So in 44 g of compound (1 mol) we have 2 moles of N
In 4.19 g of compound we would have ( 4.19 .2 ) / 44 = 0.190 moles of N
Now, we know that 1 mol of anything has NA particles so:
1 mol of N has 6.02×10²³ atoms
0.190 moles of N, would have (0.190 .NA) = 1.14×10²³
Let's verify the amount of molecules, in our compound.
First of all, let's convert the mass to moles (mass / molar mass)
4.19 g / 44 g/m = 0.095 moles
moles . NA = amount of atoms → 5.71×10²² ≅
Answer:
We have 1.15 *10^23 nitrogen atoms
Explanation:
Step 1: Data given
Mass of N2O = 4.19 grams
Number of N2O molecules = 5.73 *10^22 molecules
Molar mass = 44.01 g/mol
Step 2: Calculate moles N2O
Moles N2O = mass N2O / molar mass N2O
Moles N2O = 4.19 grams / 44.01 g/mol
Moles N2O = 0.0952 moles
Step 3: Calculate moles nitrogen
For each mol N2O we have 2 moles of Nitrogen
For 0.0952 moles N2O we have 2*0.0952 = 0.1904 moles nitrogen
Step 4: Calculate atoms nitrogen
Number of nitrogen atoms = moles * number of Avogadro
Number of nitrogen atoms = 0.1904 moles * 6.022*10^23
Number of nitrogen atoms = 1.15 *10^23 atoms
We have 1.15 *10^23 nitrogen atoms
