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How many atoms of Iodine are in 56.243 gI?

A. 1.20 x 10^23
B. 2.40 x 10^23
C. 6.022 x 10^23
D. 3.01 x 10^23

User Hangon
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1 Answer

3 votes

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.

User MTahir
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