what is the mass in grams of 1.32 x 10^20 uranium atoms
mols U atoms = 1.32E20/6.02E23 = ?
grams = mols x atomic mass.
3.95x10^-22
To find the mass of 1.32 x 10^20 uranium atoms, we'll need to use the molar mass of uranium and convert it into grams.
1. Start by finding the molar mass of uranium. The molar mass of an element is the mass of one mole of atoms of that element. The molar mass of uranium (U) is approximately 238.03 g/mol.
2. Convert the number of atoms into moles. 1.32 x 10^20 atoms is equivalent to 1.32 x 10^20 / (6.022 x 10^23) ≈ 2.19 x 10^-4 moles. (Note: Avogadro's number is 6.022 x 10^23, which represents the number of atoms or molecules in one mole of a substance.)
3. Multiply the number of moles by the molar mass to find the mass in grams.
2.19 x 10^-4 moles x 238.03 g/mol ≈ 5.22 x 10^4 grams.
Therefore, the mass in grams of 1.32 x 10^20 uranium atoms is approximately 5.22 x 10^4 grams.