Answer :

Final answer:

In 600 grams of iron, there are approximately 6.47x10^24 atoms. This is found by first converting grams of iron to moles using the molar mass of iron, and then converting moles to atoms using Avogadro's number.

Explanation:

The question is asking about the number of atoms present in a certain amount of iron. To find this, we use the concept of the mole from chemistry. We know that the molar mass of iron (Fe) is approximately 55.85 g/mol, meaning that one mole of iron has a mass of 55.85 g. Also, one mole of any substance contains Avogadro's number of entities (6.022x10^23), in this case atoms.

Given this, to find the number of atoms in 600 grams of iron, we will need to first convert grams of iron to moles of iron, using the molar mass of iron, and then convert moles of iron to atoms of iron, using Avogadro's number. The calculation goes like this:

  1. First calculate the number of moles: (6.00*10^2 g) / (55.85 g/mol) = 10.74 mol of Fe.
  2. Then convert moles to atoms by multiplying by Avogadro's number: (10.74 mol) * (6.022x10^23 atoms/mol) = 6.47x10^24 atoms of Fe.

Therefore, in 600 grams of Fe, there are approximately 6.47x10^24 atoms of iron.

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