Approximately how many atoms of carbon are present in a 120 gram sample of carbon (assume the sample is pure \(^{12}\)C)?

• A. 6.02 × 10^{23} atoms
• B. 2.41 × 10^{25} atoms
• C. 1.00 × 10^{24} atoms
• D. 6.02 × 10^{24} atoms

Answer: (D)

Verified step by step guidance

1. Identify the molar mass of the carbon isotope given, which is \(^{12}\)C. The molar mass of \(^{12}\)C is 12 grams per mole.
2. Calculate the number of moles of carbon in the 120 gram sample using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\). Substitute the values to get \(\text{moles} = \frac{120}{12}\).
3. Use Avogadro's number, which is \$6.02 \times 10^{23}\( atoms per mole, to convert moles of carbon to atoms. The formula is: \)\text{number of atoms} = \text{moles} \times 6.02 \times 10^{23}$.
4. Multiply the number of moles calculated in step 2 by Avogadro's number to find the total number of carbon atoms in the sample.
5. Express the final answer in scientific notation to match the format of the options provided.