Final answer:
To convert 1.85 g of bismuth (Bi) to atoms, calculate the moles using the atomic weight of bismuth and then use Avogadro's number to find the atoms. The correct calculation gives approximately 5.33 × 10²± atoms of Bi.
Step-by-step explanation:
To convert 1.85 g of bismuth (Bi) to atoms, we need to use Avogadro's number and the atomic weight of bismuth.
The atomic weight of bismuth is approximately 209 g/mol.
The conversion process involves the following steps:
Calculate the number of moles of Bi in 1.85 g:
Moles of Bi = mass (g) / atomic weight (g/mol)
Moles of Bi = 1.85 g / 209 g/mol = 0.00885 mol
Use Avogadro's number to convert moles to atoms:
Atoms of Bi = moles of Bi × Avogadro's number (6.022 × 10²³ atoms/mol)
Atoms of Bi = 0.00885 mol × 6.022 × 10²³ atoms/mol
Calculate the total number of atoms:
Atoms of Bi = 5.32947 × 10²± atoms
The result does not match with any of the provided options (A, B, C, D).
The correct amount of bismuth atoms is approximately 5.33 × 10²±, which may suggest a typo or miscalculation in the question or answer choices.
Make sure to double-check your calculations if you encounter this type of issue on a test or assignment.