Final answer:
By dividing the mass of iodine by its atomic mass and then multiplying by Avogadro's number, we find that there are approximately 2.67 x 10^22 atoms of iodine in 56.243 g, which doesn't match any of the provided options.
Step-by-step explanation:
To find out how many atoms of iodine are in 56.243 g of iodine, we use Avogadro's number and the fact that the atomic mass of iodine (I) is 127 g/mol. First, we need to calculate the number of moles of iodine:
Number of moles = Mass in grams ÷ Atomic mass = 56.243 g I ÷ 127 g/mol ≈ 0.443 g/mol.
Next, we calculate the number of atoms using Avogadro's number (6.022 x 1023 atoms/mol):
Number of iodine atoms = 0.443 mol x 6.022 x 1023 atoms/mol ≈ 2.67 x 1022 atoms.
None of the given options matches this result, so it seems there might be a miscalculation or typographical error in the options provided.