N$_2$ + 3H$_2$ $ ightleftharpoons$ 2NH$_3$ In the reaction above, 5 mol N$_2$ and 12 mol H$_2$ react to produce ammonia. Only [ans] NH$_3$ are produced, because [Select ] is the limiting reactant and therefore runs out first thus stopping the production of any more products.
Added by Jose L.
Close
Step 1
Step 1: Write out the balanced chemical equation for the reaction between nitrogen gas (N2) and hydrogen gas (H2) to produce ammonia (NH3): N2 + 3H2 -> 2NH3 Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 73 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Adi S.
In the balanced equation below, determine the limiting reactant and amount in mol of NH3 (g) produced if 2.50 g of H2 (g) and 4.50 g of N2 (g) are combined. The molar mass of H2 (g) is 2 g/mol and the molar mass of N2 (g) is 28 g/mol. 3H2 (g) + N2 (g) -> 2NH3 (g) H2 is the limiting reactant and 0.833 mol of NH3 (g) is produced. N2 is the limiting reactant and 0.833 mol of NH3 (g) is produced. N2 is the limiting reactant and 0.321 mol of NH3 (g) is produced. H2 is the limiting reactant and 0.321 mol of NH3 (g) is produced.
David C.
When the reaction N2 + 3H to 2NH3 is complete how many NH3 are produced what’s the limiting reactant
Susan H.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD