What is the number of atoms in a sample of nickel weighing 11.74 g?

What is the number of atoms in a sample of nickel weighing 11.74 g?

• A. 1.174 x 10^23 atoms
• B. 1.205 x 10^23 atoms
• C. 1.869 x 10^23 atoms
• D. 3.256 x 10^23 atoms

Answer: (B)

To determine the number of atoms in a sample of nickel weighing 11.74 g, first, we need to use the molar mass of nickel to convert grams to moles. The molar mass of nickel (Ni) is approximately 58.69 g/mol. By dividing the mass of the nickel sample by its molar mass, we find the number of moles: \[ \text{Moles of Ni} = \frac{11.74 \, \text{g}}{58.69 \, \text{g/mol}} \approx 0.199 \, \text{moles} \] Next, we apply Avogadro's number to convert moles to atoms. Avogadro's number, which is approximately \(6.022 \times 10^{23}\) atoms/mol, tells us how many atoms are present in one mole. Now, multiply the moles of nickel by Avogadro's number: \[ \text{Number of atoms} = 0.199 \, \text{moles} \times 6.022 \times 10^{23} \, \text{atoms/mole} \approx 1.205 \times

To determine the number of atoms in a sample of nickel weighing 11.74 g, first, we need to use the molar mass of nickel to convert grams to moles. The molar mass of nickel (Ni) is approximately 58.69 g/mol.

By dividing the mass of the nickel sample by its molar mass, we find the number of moles:

[

\text{Moles of Ni} = \frac{11.74 , \text{g}}{58.69 , \text{g/mol}} \approx 0.199 , \text{moles}

]

Next, we apply Avogadro's number to convert moles to atoms. Avogadro's number, which is approximately (6.022 \times 10^{23}) atoms/mol, tells us how many atoms are present in one mole.

Now, multiply the moles of nickel by Avogadro's number:

[

\text{Number of atoms} = 0.199 , \text{moles} \times 6.022 \times 10^{23} , \text{atoms/mole} \approx 1.205 \times