Final answer:
There are 0.933 moles of NH₃ produced when 1.4 moles of H₂ react. This is determined by the stoichiometric ratio of 2 moles of NH₃ to 3 moles of H₂ from the balanced chemical equation.
Step-by-step explanation:
The question concerns stoichiometry, a section of Chemistry that involves the calculation of reactants and products in chemical reactions. Specifically, the query is about how many moles of NH₃ (ammonia) can be produced from a given amount of H₂ (hydrogen gas) in the presence of excess nitrogen gas according to the balanced chemical equation:
N₂(g) + 3H₂(g) → 2NH₃(g)
This equation indicates that 3 moles of hydrogen gas are needed to produce 2 moles of ammonia. To find out how many moles of ammonia will be produced from 1.4 moles of hydrogen, we use the ratio derived from the balanced equation: 2 moles of NH₃ per 3 moles of H₂. Using a simple cross-multiplication, we determine that 1.4 moles of hydrogen will produce:
(2 moles NH₃ / 3 moles H₂) × 1.4 moles H₂
Calculating this gives us 0.933 moles of NH₃ (ammonia). However, in a real experimental situation, one must remember that the yield may vary due to factors like reaction efficiency and product recovery. Nonetheless, for the stoichiometry problem provided, 1.4 mol of hydrogen would theoreticall produce 0.933 moles of ammonia.