A sample of copper has a mass of 63.5 g. How many atoms of copper are present in the sample?

• A. 9.54 × 10^{22} atoms
• B. 1.00 × 10^{24} atoms
• C. 6.02 × 10^{23} atoms
• D. 3.02 × 10^{23} atoms

Answer: (C)

Verified step by step guidance

1. Identify the given information: the mass of the copper sample is 63.5 g.
2. Recall the molar mass of copper (Cu), which is approximately 63.5 g/mol. This means 1 mole of copper atoms has a mass of 63.5 g.
3. Calculate the number of moles of copper in the sample using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).
4. Use Avogadro's number, \$6.022 \times 10^{23}\( atoms/mol, to convert moles of copper to number of atoms with the formula: \)\text{number of atoms} = \text{moles} \times 6.022 \times 10^{23}$ atoms/mol.
5. Combine the steps to find the total number of copper atoms in the 63.5 g sample without calculating the final value.