Answer:
There are approximately 3.944 x 10^21 atoms in 1.230g of Cu(NO3)2.
Step-by-step explanation:
To determine the number of atoms in 1.230g of Cu(NO3)2, we need to first calculate the number of moles of Cu(NO3)2 in 1.230g, using its molar mass.
The molar mass of Cu(NO3)2 can be calculated as follows:
Cu: 1 atom x 63.55 g/mol = 63.55 g/mol
N: 2 atoms x 14.01 g/mol = 28.02 g/mol
O: 6 atoms x 16.00 g/mol = 96.00 g/mol
Total molar mass of Cu(NO3)2 = 63.55 + 28.02 + 96.00 = 187.57 g/mol
Now, we can calculate the number of moles of Cu(NO3)2:
moles = mass / molar mass
moles = 1.230 g / 187.57 g/mol = 0.006558 moles
Finally, we can use Avogadro's number (6.022 x 10^23 atoms/mole) to convert the number of moles to atoms:
number of atoms = moles x Avogadro's number
number of atoms = 0.006558 moles x 6.022 x 10^23 atoms/mole = 3.944 x 10^21 atoms
Therefore, there are approximately 3.944 x 10^21 atoms in 1.230g of Cu(NO3)2.