Question

Consider the reaction N₂(g) + 3H₂(g) → 2NH₃(g).

1) If hydrogen gas is added to the above system at equilibrium, which direction will the reaction shift?
2) If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?
3) If nitrogen is removed from the system at equilibrium, what will happen to the hydrogen (H₂) concentration?
4) The production of ammonia is an endothermic reaction. Will heating the equilibrium system increase or decrease the amount of ammonia produced?
5) If we use a catalyst, which way will the reaction shift?

Answer 1

Adding H2 or N2 will shift the reaction toward products, increasing NH3 production. Removing N2 decreases H2 and NH3. Heating an endothermic reaction will increase NH3, while a catalyst speeds up reaching equilibrium without shifting it.

Step-by-step explanation:

Understanding Chemical Equilibrium Shifts

Leveraging Le Chatelier's Principle helps us predict how a chemical reaction at equilibrium responds to changes in conditions.

1. Adding hydrogen gas (H2) to the system at equilibrium will cause the reaction to shift toward the products, thereby increasing the production of ammonia (NH3).
2. If nitrogen (N2) is added to the system at equilibrium, the concentration of NH3 will increase as the reaction shifts in the forward direction to use up the added N2.
3. Removing N2 from the system will lead to an increase in the reaction shifting towards the reactants, causing a decrease in NH3 production and therefore reducing the hydrogen (H2) concentration.
4. Since the production of ammonia is endothermic, heating the system will drive the equilibrium towards the products side, thus increasing NH3 production.
5. Using a catalyst does not shift the reaction in any direction; it simply speeds up the reaction rate equally in both directions, allowing equilibrium to be reached more quickly.