Question

If you had 1.37 x 1022 atoms of lead (Pb), what would the mass of that sample be?

Answer 1

A sample of 1.37 x 10^22 atoms of lead (Pb) would have a mass of approximately 4.7122 grams, calculating using Avogadro's number and the molar mass of lead.

Step-by-step explanation:

To calculate the mass of a sample containing 1.37 x 1022 atoms of lead (Pb), we need to use Avogadro's number (6.022 x 1023 atoms/mol) that relates the number of atoms to moles, and the molar mass of lead. Given that the atomic mass of lead (Pb) is 207.2 g/mol, we can perform the following calculation:

1. First, determine the number of moles by dividing the number of atoms by Avogadro's number:
2. Number of moles = 1.37 x 1022 atoms / 6.022 x 1023 atoms/mol = 0.02275 mol.
3. Then, multiply the number of moles by the molar mass of lead to find the mass:
4. Mass = 0.02275 mol x 207.2 g/mol = 4.7122 grams.

Therefore, a sample of 1.37 x 1022 atoms of lead weighs approximately 4.7122 grams.