What is the mass of sodium metal that contains 4.653 × 10^{19} Na atoms? (Atomic mass of Na = 22.99 g/mol)

• A. 0.0018 g
• B. 0.18 g
• C. 1.8 g
• D. 0.018 g

Answer: (A)

Verified step by step guidance

1. Identify the given information: the number of sodium atoms is \$4.653 \times 10^{19}$ atoms, and the atomic mass of sodium (Na) is 22.99 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 sodium atoms by dividing the given number of atoms by Avogadro's number using the formula: \(\text{moles of Na} = \frac{4.653 \times 10^{19} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mol}}\).
4. Convert the moles of sodium to mass by multiplying the moles by the atomic mass of sodium: \(\text{mass of Na} = \text{moles of Na} \times 22.99 \text{ g/mol}\).
5. The result from the previous step will give the mass of sodium metal containing \$4.653 \times 10^{19}$ atoms.