How many carbon atoms are present in 15.0 grams of graphite (pure carbon)? (Atomic mass of carbon = 12.01 g/mol)

• A. 1.25 × 10^{24} atoms
• B. 5.02 × 10^{22} atoms
• C. 3.01 × 10^{23} atoms
• D. 7.52 × 10^{23} atoms

Answer: (D)

Verified step by step guidance

1. Identify the given information: mass of graphite = 15.0 g, atomic mass of carbon = 12.01 g/mol.
2. Calculate the number of moles of carbon atoms in 15.0 g of graphite using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}} = \frac{15.0}{12.01}\).
3. Recall that 1 mole of any substance contains Avogadro's number of particles, which is \$6.022 \times 10^{23}$ atoms/mol for carbon atoms.
4. Calculate the total number of carbon atoms by multiplying the moles of carbon by Avogadro's number: \(\text{number of atoms} = \text{moles} \times 6.022 \times 10^{23}\).
5. Express the final answer in scientific notation to compare with the given options.