A pure silver ring contains 2.80 × 10^{22} silver atoms. How many moles of silver atoms does it contain?

• A. 0.0465 mol
• B. 0.168 mol
• C. 4.65 mol
• D. 1.68 × 10^{-2} mol

Answer: (A)

Verified step by step guidance

1. Identify the given quantity: the number of silver atoms in the ring, which is \$2.80 \times 10^{22}$ atoms.
2. Recall the definition of a mole: one mole contains Avogadro's number of particles, which is \$6.022 \times 10^{23}$ atoms/mol.
3. Set up the conversion from atoms to moles using the relationship: \(\text{moles} = \frac{\text{number of atoms}}{\text{Avogadro's number}}\).
4. Substitute the given values into the formula: \(\text{moles} = \frac{2.80 \times 10^{22}}{6.022 \times 10^{23}}\).
5. Perform the division to find the number of moles of silver atoms in the ring.