Final answer:
To find the moles of N₂ required, convert 3.53 grams of H₂ to moles and then use the mole ratio from the balanced equation. The answer is approximately 0.584 moles of N₂, which is closest to option C.
Step-by-step explanation:
The question asks for the number of moles of N₂ that are required to react with 3.53 grams of H₂ according to the balanced chemical equation N₂ + 3H₂ → 2NH₃. Firstly, we need to convert grams of H₂ to moles using the molar mass of H₂ (approximately 2.02 g/mol). Calculating this gives:
(3.53 g H₂) / (2.02 g/mol) = 1.747 moles H₂
According to the stoichiometry of the balanced equation, it takes 3 moles of H₂ to react with 1 mole of N₂. Therefore, we can calculate the moles of N₂ needed using the ratio from the equation:
1.747 moles H₂ × (1 mole N₂ / 3 moles H₂) = 0.58233 moles N₂
The closest answer choice to this calculation is option C, 0.584 moles of N₂.