![\boxed {\boxed {\sf 0.566 \ mol \ Fe}}](/tpl/images/1398/9910/7b08b.png)
Explanation:
We are asked to convert a number of atoms to moles.
We can convert atoms to moles using Avogadro's Number, which is 6.022 × 10²³. This is the number of particles (atoms, molecules, formula units, etc.) in 1 mole of a substance. In this problem, the particles are atoms of iron (Fe). There are 6.022 ×10²³ atoms of iron in 1 mole of iron.
We use dimensional analysis to convert atoms to moles. This involves setting up ratios. Use Avogadro's Number and the underlined information to make a ratio.
![\frac {6.022 \times 10^{23}\ atoms \ Fe}{1 \ mol \ Fe}](/tpl/images/1398/9910/66a54.png)
We are converting 3.41 × 10²³ atoms of iron to moles, so we multiply by this value.
![3.41 \times 10^{23} \ atoms \ Fe *\frac {6.022 \times 10^{23}\ atoms \ Fe}{1 \ mol \ Fe}](/tpl/images/1398/9910/fd4c7.png)
Flip the ratio. It stays equivalent, but it allows the units of atoms of iron to cancel.
![3.41 \times 10^{23} \ atoms \ Fe *\frac{1 \ mol \ Fe} {6.022 \times 10^{23}\ atoms \ Fe}](/tpl/images/1398/9910/55580.png)
![3.41 \times 10^{23}*\frac{1 \ mol \ Fe} {6.022 \times 10^{23}}](/tpl/images/1398/9910/2bcf3.png)
![\frac{3.41 \times 10^{23}} {6.022 \times 10^{23}} \ mol \ Fe](/tpl/images/1398/9910/a005a.png)
![0.5662570575\ mol \ Fe](/tpl/images/1398/9910/c97ff.png)
The original measure ment of iron atoms ( 3.41 × 10²³ ) has 3 significant figures, so our answer must have the same. For the number we calculated, that is the thousandths place. The 2 in the ten-thousandths place ( 0.5662570575) tells us to leave the 6 in the thousandths place.
![0.566 \ mol \ Fe](/tpl/images/1398/9910/5832e.png)
3.41 × 10²³ atoms of iron is equal to approximately 0.566 moles of iron.