Question

. Most of the industrial ammonia today is produced via the Haber Process. The Chemical reaction is one we’ve seen many times now:
N_2 (g)+3H_2 (g)⟶2NH_3 (g)
If 20 moles of ammonia (NH_3) are needed for a particular process, how many moles of diatomic Nitrogen (N_2) are needed?

Answer 1

According to the balanced chemical equation, 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3.

Therefore, the molar ratio between N2 and NH3 is 1:2. This means that for every 2 moles of NH3 produced, 1 mole of N2 is needed.

Since we need 20 moles of NH3, we can calculate the amount of N2 needed using the ratio:

Number of moles of N2 = (20 moles of NH3) / (2 moles of NH3 per 1 mole of N2)
= 20 moles of NH3 / 2
= 10 moles of N2

Therefore, 10 moles of diatomic Nitrogen (N2) are needed to produce 20 moles of ammonia (NH3).