In the reaction N_2 + 3H_2 → 2NH_3, how many moles of hydrogen gas (H_2) are required to completely react with 0.850 moles of nitrogen gas (N_2)?

• A. 2.55 moles
• B. 0.850 moles
• C. 1.70 moles
• D. 3.40 moles

Answer: (A)

Verified step by step guidance

1. Identify the balanced chemical equation: \(\mathrm{N_2 + 3H_2 \rightarrow 2NH_3}\).
2. Note the mole ratio between nitrogen gas (\(\mathrm{N_2}\)) and hydrogen gas (\(\mathrm{H_2}\)) from the balanced equation, which is 1 mole of \(\mathrm{N_2}\) reacts with 3 moles of \(\mathrm{H_2}\).
3. Given the amount of nitrogen gas is 0.850 moles, set up a proportion to find the moles of hydrogen gas required: \(\mathrm{0.850\ moles\ N_2 \times \frac{3\ moles\ H_2}{1\ mole\ N_2}}\).
4. Multiply the given moles of \(\mathrm{N_2}\) by the mole ratio to calculate the moles of \(\mathrm{H_2}\) needed for complete reaction.
5. The result from the multiplication will give the number of moles of hydrogen gas required to completely react with 0.850 moles of nitrogen gas.