In the reaction N_2 + 3H_2 ightarrow 2NH_3, how many grams of ammonia (NH_3) are produced when 1.0 mole of nitrogen gas (N_2) reacts completely with excess hydrogen gas?

• A. 34 grams
• B. 17 grams
• C. 2 grams
• D. 30 grams

Answer: (A)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \(\mathrm{N_2 + 3H_2 \rightarrow 2NH_3}\).
2. Identify the mole ratio between nitrogen gas (\(\mathrm{N_2}\)) and ammonia (\(\mathrm{NH_3}\)) from the balanced equation. For every 1 mole of \(\mathrm{N_2}\), 2 moles of \(\mathrm{NH_3}\) are produced.
3. Calculate the moles of ammonia produced when 1.0 mole of \(\mathrm{N_2}\) reacts completely using the mole ratio: \(\text{moles of } NH_3 = 1.0 \times 2 = 2.0\) moles.
4. Determine the molar mass of ammonia (\(\mathrm{NH_3}\)) by adding the atomic masses: nitrogen (14 g/mol) + 3 hydrogens (3 × 1 g/mol) = 17 g/mol.
5. Calculate the mass of ammonia produced by multiplying the moles of ammonia by its molar mass: \(\text{mass of } NH_3 = 2.0 \times 17 \text{ g/mol}\).