How many atoms of iron (Fe) are present in a sample containing 7.38 mol Fe?

• A. 1.23 × 10^{25} atoms
• B. 7.38 × 10^{23} atoms
• C. 4.44 × 10^{24} atoms
• D. 6.02 × 10^{24} atoms

Answer: (C)

Verified step by step guidance

1. Identify the given quantity: 7.38 moles of iron (Fe).
2. Recall that 1 mole of any substance contains Avogadro's number of particles (atoms, molecules, etc.), which is \$6.022 \times 10^{23}$ particles per mole.
3. Set up the calculation to find the number of atoms by multiplying the number of moles by Avogadro's number: \(\text{Number of atoms} = 7.38 \text{ mol} \times 6.022 \times 10^{23} \frac{\text{atoms}}{\text{mol}}\).
4. Perform the multiplication of the numerical values and combine the powers of ten according to the rules of exponents.
5. Express the final answer in scientific notation to represent the total number of iron atoms in the sample.