How many atoms of sulfur are present in 4.30 grams of carbon disulfide (CS_2)?

• A. 2.16 × 10^{23} atoms
• B. 1.08 × 10^{23} atoms
• C. 3.61 × 10^{22} atoms
• D. 6.02 × 10^{22} atoms

Answer: (B)

Verified step by step guidance

1. Identify the molecular formula of carbon disulfide, which is CS\_2, meaning each molecule contains 2 atoms of sulfur.
2. Calculate the molar mass of CS\_2 by adding the atomic masses: Carbon (C) is approximately 12.01 g/mol and Sulfur (S) is approximately 32.07 g/mol. So, molar mass = 12.01 + 2 \times 32.07 g/mol.
3. Determine the number of moles of CS\_2 in 4.30 grams by using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).
4. Calculate the total number of molecules of CS\_2 by multiplying the moles by Avogadro's number (\$6.022 \times 10^{23}\( molecules/mol): \)\text{molecules} = \text{moles} \times 6.022 \times 10^{23}$.
5. Since each molecule contains 2 sulfur atoms, multiply the total number of molecules by 2 to find the total number of sulfur atoms: \(\text{S atoms} = 2 \times \text{molecules}\).