Question

Nitrogen and hydrogen gases react to form ammonia gas via the following reaction:

N2(g)+3H2(g)→2NH3(g)
At a certain temperature and pressure, 1.9 L of N2 reacts with 5.7 L of H2.

If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?

Answer 1

When 1.9 L of N₂ gas reacts with 5.7 L of H₂ gas, 3.8 L of NH₃ gas are produced, following the balanced chemical equation N₂(g) + 3 H₂(g) → 2 NH₃(g) and Avogadro's law.

Step-by-step explanation:

The question asks about the reaction between nitrogen (N₂) and hydrogen (H₂) gases to produce ammonia (NH₃) gas, and specifically, how to determine the volume of ammonia gas produced when given the volumes of the reactants nitrogen and hydrogen. According to Avogadro's law, under the same conditions of temperature and pressure, equal volumes of gases contain the same number of molecules. Based on the balanced chemical equation N₂(g) + 3 H₂(g) → 2 NH₃(g), one volume unit of N₂ reacts with three volume units of H₂ to produce two volume units of NH₃.

Given that 1.9 L of N₂ reacts with 5.7 L of H₂, and because the ratio of hydrogen to nitrogen is exactly 3:1 as required by the balanced chemical equation, all of the reactants will be consumed. Therefore, for 1.9 L of N₂, we will obtain twice that volume in NH₃, which is 3.8 L of NH₃.

Answer 2

1mol N2 + 3mol H2 → 2mol NH3
Because you are dealing with gases, at the same temperature and pressure you can say:
1volume N2 + 3 volumes H2 → 2 volumes NH3
OR: 4 volumes reactants = 2 volumes products.
You have 1.9+5.7 = 7.6 volumes reactants, which must give 7.6/2 = 3.8 volumes of NH3
Answer: 3.8 litres of NH3 will be formed