What is the mass in grams of 1.900 × 10^{24} iodine atoms? (Atomic mass of iodine = 126.90 g/mol)

• A. 63.5 g
• B. 240 g
• C. 401 g
• D. 126.9 g

Answer: (C)

Verified step by step guidance

1. Identify the given information: the number of iodine atoms is \$1.900 \times 10^{24}$ atoms, and the atomic mass of iodine is 126.90 g/mol.
2. Recall that 1 mole of any substance contains Avogadro's number of atoms, which is \$6.022 \times 10^{23}$ atoms/mol.
3. Calculate the number of moles of iodine atoms by dividing the given number of atoms by Avogadro's number: \(\text{moles} = \frac{1.900 \times 10^{24} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mol}}\).
4. Use the atomic mass to convert moles to grams: \(\text{mass (g)} = \text{moles} \times 126.90 \text{ g/mol}\).
5. Combine the calculations from steps 3 and 4 to find the mass in grams of the given iodine atoms.