What mass of sulfur (S) contains exactly 4.7 × 10^{22} atoms of sulfur?

• A. 1.5 g
• B. 0.8 g
• C. 4.7 g
• D. 2.5 g

Answer: (D)

Verified step by step guidance

1. Identify the given quantity: the number of sulfur atoms, which is \$4.7 \times 10^{22}$ atoms.
2. Recall the relationship between moles and number of atoms: 1 mole contains Avogadro's number of atoms, which is \$6.022 \times 10^{23}$ atoms/mol.
3. Calculate the number of moles of sulfur atoms using the formula: \(\text{moles} = \frac{\text{number of atoms}}{6.022 \times 10^{23}}\).
4. Use the molar mass of sulfur (S), which is approximately 32.07 g/mol, to convert moles to mass with the formula: \(\text{mass} = \text{moles} \times 32.07\) g/mol.
5. Substitute the moles calculated in step 3 into the formula in step 4 to find the mass of sulfur containing \$4.7 \times 10^{22}$ atoms.