Question

In a 3.0-L vessel, the following equilibrium partial pressures are measured: N₂, 190 torr; H₂, 317 torr; NH₃, 1.00 × 10³ torr. Write the balanced equation

Answer 1

The balanced chemical equation for nitrogen reacting with hydrogen to form ammonia is N₂(g) + 3H₂(g) ⇒ 2NH₃(g). Removing H₂ will cause the partial pressures of H₂ and NH₃ to decrease, and the partial pressure of N₂ to increase. The new partial pressures can be calculated using the equilibrium constant and the stoichiometry of the reaction.

Step-by-step explanation:

The balanced chemical equation for the reaction given in your question, where nitrogen (N₂) reacts with hydrogen (H₂) to form ammonia (NH₃), is N₂(g) + 3H₂(g) ⇒ 2NH₃(g). Regarding the effect of removing H₂ from the system, according to Le Chatelier's Principle, if a reactant (like H₂) is removed, the equilibrium will shift to the left, toward the formation of more reactants.

Consequently, the partial pressure of H₂ would decrease, the partial pressure of NH₃ decreases as well, and the partial pressure of N₂ would increase until a new equilibrium is established.

With the equilibrium constant (Kc) being 5.0 at a given temperature, the partial pressures can be recalculated using the new partial pressure of N₂, which is 250 torr. The partial pressures of H₂ and NH₃ can be determined by the stoichiometry of the reaction and the equilibrium constant.