When 1 mole of N₂ and 1 mole of H₂ are allowed to react to form ammonia, H₂ is the limiting reagent and only a small amount of NH₃ can form.

Step 1: Use the balanced equation

The balanced equation for ammonia synthesis is:

N2+3H2→2NH3\text{N}_2+3\text{H}_2\rightarrow 2\text{NH}_3N2​+3H2​→2NH3​

This shows that 1 mole of N₂ needs 3 moles of H₂ to react completely.

Step 2: Compare required vs available moles

  • You have:
    • N₂ = 1 mole
    • H₂ = 1 mole
  • Stoichiometric requirement:
    • For 1 mole N₂ → need 3 moles H₂
    • But only 1 mole H₂ is present, so H₂ is limiting and N₂ is in excess.

Step 3: Calculate moles of NH₃ formed

From the balanced equation:

  • 3 moles H₂ → 2 moles NH₃

So for 1 mole H₂:

NH3=23 mole\text{NH}_3=\frac{2}{3}\text{ mole}NH3​=32​ mole

Therefore, when 1 mole of N₂ and 1 mole of H₂ react:

  • Maximum NH₃ formed = 23\frac{2}{3}32​ mole
  • H₂ is completely consumed, and some N₂ is left unreacted.

So, the key result: 2 3\frac{2}{3}32​ mole of NH₃ can be produced from 1 mole N₂ and 1 mole H₂.