To calculate the mass of 3.2 multiplied by 10^23 atoms of carbon, we need to know the atomic mass of carbon. The atomic mass of carbon (C) is approximately 12.01 grams per mole (g/mol).
We can use the concept of Avogadro's number to convert the given number of atoms to moles, and then multiply by the molar mass of carbon to obtain the mass.
1 mole of carbon contains Avogadro's number of atoms, which is approximately 6.022 x 10^23 atoms.
Given: Number of atoms of carbon = 3.2 x 10^23
First, let's calculate the number of moles:
Number of moles = (Number of atoms) / (Avogadro's number) = (3.2 x 10^23 atoms) / (6.022 x 10^23 atoms/mol) ≈ 0.531 moles (approximately)
Now, let's calculate the mass:
Mass = Number of moles x Molar mass = 0.531 moles x 12.01 g/mol ≈ 6.38 grams
Therefore, the mass of 3.2 multiplied by 10^23 atoms of carbon is approximately 6.38 grams.