the mass of an individual atom of fluorine is 19 amu. how many atoms would weigh a total of 1.7455x10-3g of this element if the mass of 1 amu is 1.6650x10-24
Divide 1.7455x10-3 g by the mass of one F atom, which is 19*1.6650x10-24 g
That will give you the number of atoms.
i got 1.812e-25 but it says that not the correct answer
it didn't work
1.7455e-3/(19*1.6650e-24) is not 1.812e-25
ty
To calculate the number of atoms that would weigh a total of 1.7455x10^-3g of fluorine, you can use the following steps:
Step 1: Calculate the number of moles:
To convert the given mass (1.7455x10^-3g) of fluorine to moles, use the formula:
moles = mass / molar mass
Given:
mass = 1.7455x10^-3g
molar mass = 19 amu = 19 * 1.6650x10^-24g
Substituting the values, we get:
moles = (1.7455x10^-3g) / (19 * 1.6650x10^-24g)
Step 2: Calculate the number of atoms:
To convert moles to the number of atoms, use Avogadro's number (6.0221x10^23 mol^-1). The number of atoms can be calculated using the formula:
number of atoms = moles * Avogadro's number
Substituting the values, we get:
number of atoms = moles * 6.0221x10^23
Now, let's calculate the number of atoms:
moles = (1.7455x10^-3g) / (19 * 1.6650x10^-24g)
≈ 5.2801x10^20 mol
number of atoms = (5.2801x10^20 mol) * (6.0221x10^23 mol^-1)
≈ 3.177x10^44 atoms
Therefore, approximately 3.177x10^44 atoms would weigh a total of 1.7455x10^-3g of fluorine.