Question

The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) -> 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?

Answer 1

In Haber process, N₂ reacts with H₂ and produces NH₃. The balanced equation for the Haber process is 
                          N₂(g) + 3H₂(g) → 2NH₃(g)
The stoichiometric ratio between H₂ and N₂ is 3 : 1
This means, reacted moles of N₂ = reacted moles of H₂ / 3 
Hence moles of N₂ = 9.0 mol / 3
                                = 3.0 mol

Hence, 3.0 moles of N₂ is needed to react with 9.0 moles of  H₂.

Answer 2

The number of mole of nitrogen gas, N₂ required for the reaction is 3 moles.

We'll begin obtaining the number of mole of N₂ and H₂ that reacted from the balanced equation.

N₂(g) + 3H₂(g) → 2NH₃(g)

From the balanced equation above,

3 moles of H₂ required 1 mole of N₂.

With the above information in mind, we can obtain the number of mole of N₂ required to react with 9 moles of H₂. This can be obtained as follow:

From the balanced equation above,

3 moles of H₂ required 1 mole of N₂.

Therefore,

9 moles of H₂ will require = 9/3 = 3 moles of N₂.

Thus, 3 moles of N₂ are required for the reaction.

Learn more about stoichiometry:

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