How many silver atoms are present in a 33.0 g bar of silver (Ag)? (Atomic mass of Ag = 107.9 g/mol)

• A. 3.08 × 10^{23} atoms
• B. 3.08 × 10^{24} atoms
• C. 1.84 × 10^{24} atoms
• D. 1.84 × 10^{23} atoms

Answer: (C)

Verified step by step guidance

1. Identify the given information: mass of silver (Ag) is 33.0 g, and the atomic mass of silver is 107.9 g/mol.
2. Calculate the number of moles of silver using the formula: \(\text{moles of Ag} = \frac{\text{mass of Ag}}{\text{atomic mass of Ag}} = \frac{33.0\ \text{g}}{107.9\ \text{g/mol}}\).
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 number of silver atoms by multiplying the moles of silver by Avogadro's number: \(\text{number of atoms} = \text{moles of Ag} \times 6.022 \times 10^{23}\).
5. Express the final answer in scientific notation to match the given options.