calculate mass of8.22*10^23atoms of rubidium
The molar mass of rubidium (Rb) is approximately 85.47 g/mol.
We can use this to calculate the mass of one mole of Rb atoms:
1 mol of Rb atoms = 85.47 g
Now, we want to calculate the mass of 8.22*10^23 Rb atoms, which is equivalent to:
(8.22*10^23 atoms) x (1 mol/6.022*10^23 atoms) x (85.47 g/mol)
Simplifying this expression, we get:
= (8.22*85.47)/6.022
= 116.2 g
Therefore, the mass of 8.22*10^23 atoms of rubidium is approximately 116.2 g.
To calculate the mass of 8.22 * 10^23 atoms of rubidium, you need to know the molar mass of rubidium (Rb). The molar mass is the mass of one mole of a substance and is expressed in grams per mole (g/mol).
The molar mass of rubidium (Rb) is approximately 85.47 g/mol.
Now, you can use the Avogadro's number (6.022 * 10^23 atoms/mol) to convert the number of rubidium atoms to moles:
Number of moles = Number of atoms / Avogadro's number
= 8.22 * 10^23 atoms / (6.022 * 10^23 atoms/mol)
Number of moles ≈ 1.363 moles
Finally, you can multiply the number of moles by the molar mass to calculate the mass:
Mass = Number of moles * Molar mass
= 1.363 moles * 85.47 g/mol
Mass ≈ 116.616 g
Therefore, the mass of 8.22 * 10^23 atoms of rubidium is approximately 116.616 grams.