In the reaction forming nitrogen monoxide, what mass of nitrogen (N_2) is required to react completely with 16 grams of oxygen (O_2)?N_2 + O_2 → 2NO

• A. 28 grams
• B. 14 grams
• C. 8 grams
• D. 32 grams

Answer: (B)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \(\mathrm{N_2 + O_2 \rightarrow 2NO}\).
2. Determine the molar masses of the reactants: \(\mathrm{N_2}\) has a molar mass of approximately 28 g/mol, and \(\mathrm{O_2}\) has a molar mass of approximately 32 g/mol.
3. Convert the given mass of oxygen (16 g) to moles using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\), so \(\mathrm{moles\ of\ O_2 = \frac{16\ g}{32\ g/mol}}\).
4. Use the mole ratio from the balanced equation to find the moles of nitrogen required. According to the equation, 1 mole of \(\mathrm{N_2}\) reacts with 1 mole of \(\mathrm{O_2}\), so moles of \(\mathrm{N_2}\) needed equals moles of \(\mathrm{O_2}\).
5. Convert the moles of nitrogen back to mass using the molar mass of \(\mathrm{N_2}\): \(\mathrm{mass = moles \times molar\ mass}\).