Stoichiometry and reaction yields

Question

Given the following equation:

2 N₂ (g) + 3 H₂ (g) →→ 2 NH₃ (g)

How many moles of NH₃ are produced if 15 mol of N₂ reacts?

Answer 1

The equation that you listed is incorrectly balanced.

On the left side of the equation there are 4 nitrogens - each N₂ has 2 nitrogens and you have 2 of these N₂'s making a total of 4. On the right side of the equation, you have only 2 nitrogens. This doesn't match up. Where did the other 2 nitrogens go?

The equation SHOULD SAY:

N₂ (g) + 3H₂ (g) → 2NH₃ (g)

This correctly balanced equation shows that for each mole of N₂ there are 2 moles of NH₃ produced meaning that if you start with 15 moles of N₂, you will be able to produced 30 moles of NH₃ (given that you have enough H₂ to do so)