An aluminum can has a mass of 15.8 grams. How many aluminum atoms are in this can? (Atomic mass of Al = 26.98 g/mol)

• A. 2.83 × 10^{24} atoms
• B. 9.48 × 10^{22} atoms
• C. 6.02 × 10^{23} atoms
• D. 3.53 × 10^{23} atoms

Answer: (D)

Verified step by step guidance

1. Identify the given information: mass of aluminum can = 15.8 grams, atomic mass of aluminum (Al) = 26.98 g/mol.
2. Calculate the number of moles of aluminum in the can using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}} = \frac{15.8}{26.98}\).
3. Recall that one mole of any substance contains Avogadro's number of atoms, which is \$6.022 \times 10^{23}$ atoms/mol.
4. Calculate the total number of aluminum atoms by multiplying the moles of aluminum by Avogadro's number: \(\text{atoms} = \text{moles} \times 6.022 \times 10^{23}\).
5. Express the final answer in scientific notation to match the format of the given options.