The density of solid nickel (Ni) is 8.90 g/cm^3. How many atoms are present per cubic centimeter (cm^3) of Ni? (Atomic mass of Ni = 58.69 g/mol; Avogadro's number = 6.022 × 10^{23} atoms/mol)

• A. 1.52 × 10^{23} atoms
• B. 9.14 × 10^{22} atoms
• C. 6.58 × 10^{21} atoms
• D. 9.13 × 10^{22} atoms

Answer: (D)

Verified step by step guidance

1. Identify the given data: density of Ni = 8.90 g/cm^3, atomic mass of Ni = 58.69 g/mol, and Avogadro's number = 6.022 \times 10^{23} atoms/mol.
2. Calculate the number of moles of Ni in 1 cm^3 using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\). Here, mass is the density times volume (1 cm^3), so \(\text{moles} = \frac{8.90 \text{ g}}{58.69 \text{ g/mol}}\).
3. Use Avogadro's number to convert moles to atoms: \(\text{atoms} = \text{moles} \times 6.022 \times 10^{23} \text{ atoms/mol}\).
4. Substitute the moles calculated in step 2 into the equation in step 3 to find the number of atoms per cm^3.
5. Interpret the result and compare it with the given options to confirm the correct number of atoms per cubic centimeter of nickel.