Given 0.247 g of N_2O, how many moles of nitrogen atoms (N) are present?

• A. 0.0112 mol
• B. 0.0247 mol
• C. 0.0079 mol
• D. 0.0056 mol

Answer: (A)

Verified step by step guidance

1. Identify the molecular formula of the compound given, which is nitrous oxide, \(\mathrm{N_2O}\), containing 2 nitrogen atoms per molecule.
2. Calculate the molar mass of \(\mathrm{N_2O}\) by summing the atomic masses: \$2 \times\( atomic mass of N plus atomic mass of O, i.e., \)2 \times 14.01 + 16.00$ g/mol.
3. Convert the given mass of \(\mathrm{N_2O}\) (0.247 g) to moles of \(\mathrm{N_2O}\) using the formula: \(\text{moles of } \mathrm{N_2O} = \frac{\text{mass of } \mathrm{N_2O}}{\text{molar mass of } \mathrm{N_2O}}\).
4. Since each mole of \(\mathrm{N_2O}\) contains 2 moles of nitrogen atoms, multiply the moles of \(\mathrm{N_2O}\) by 2 to find the moles of nitrogen atoms: \(\text{moles of N} = 2 \times \text{moles of } \mathrm{N_2O}\).
5. Report the final answer as the number of moles of nitrogen atoms present in the 0.247 g sample of \(\mathrm{N_2O}\).