What is the mass, in grams, of 1.56 × 10^{21} atoms of magnesium (Mg)? (Atomic mass of Mg = 24.3 g/mol)

• A. 0.063 g
• B. 2.52 g
• C. 0.38 g
• D. 0.0063 g

Answer: (A)

Verified step by step guidance

1. Identify the given information: number of atoms of magnesium (Mg) = \$1.56 \times 10^{21}$ atoms, and atomic mass of Mg = 24.3 g/mol.
2. Recall that 1 mole of any element contains Avogadro's number of atoms, which is \$6.022 \times 10^{23}$ atoms/mol.
3. Calculate the number of moles of Mg atoms by dividing the given number of atoms by Avogadro's number using the formula: \(\text{moles} = \frac{\text{number of atoms}}{6.022 \times 10^{23}}\).
4. Convert moles of Mg to mass in grams by multiplying the moles by the atomic mass of Mg: \(\text{mass} = \text{moles} \times 24.3 \, \text{g/mol}\).
5. Combine the steps to find the mass of Mg corresponding to \$1.56 \times 10^{21}$ atoms without calculating the final value.