How many moles of nitrogen atoms (N) are present in 0.239 g of dinitrogen monoxide (N_2O)?

• A. 0.0163 mol
• B. 0.00543 mol
• C. 0.0109 mol
• D. 0.00815 mol

Answer: (A)

Verified step by step guidance

1. Identify the molecular formula of dinitrogen monoxide, which is \(\mathrm{N_2O}\), meaning each molecule contains 2 nitrogen atoms and 1 oxygen atom.
2. Calculate the molar mass of \(\mathrm{N_2O}\) by summing the atomic masses: \$2 \times\( atomic mass of N (approximately 14.01 g/mol) plus 1 \)\times\( atomic mass of O (approximately 16.00 g/mol). The formula is: \)\mathrm{Molar\ mass} = 2 \times 14.01 + 16.00$ g/mol.
3. Determine the number of moles of \(\mathrm{N_2O}\) in 0.239 g by using the formula: \(\mathrm{moles\ of\ N_2O} = \frac{\mathrm{mass\ of\ sample}}{\mathrm{molar\ mass}} = \frac{0.239\ \mathrm{g}}{\mathrm{molar\ mass\ of\ N_2O}}\).
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: \(\mathrm{moles\ of\ N} = 2 \times \mathrm{moles\ of\ N_2O}\).
5. The result from the previous step gives the number of moles of nitrogen atoms present in 0.239 g of \(\mathrm{N_2O}\).