Final answer:
To calculate the mass of a sample of bismuth containing 7.35 × 10^23 atoms, we need to use the concept of molar mass and Avogadro's number. The mass in grams of the sample is 258.86 grams.
Step-by-step explanation:
To calculate the mass of a sample of bismuth (Bi) containing 7.35 × 10^23 atoms, we need to use the concept of molar mass. The molar mass of bismuth (Bi) is 208.98 grams/mol. We can use Avogadro's number, which is 6.022 × 10^23 atoms/mol, to convert the given number of atoms to moles.
Next, we can use the molar mass to convert moles to grams. The conversion factor is 1 mole = molar mass in grams. So, the mass in grams of the sample of bismuth would be:
Mass = (Number of atoms / Avogadro's number) x Molar mass = (7.35 × 10^23 atoms / 6.022 × 10^23 atoms/mol) x 208.98 grams/mol = 258.86 grams (rounded to two decimal places).
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