The chemical reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) is at equilibrium. An experimenter injects a small amount of N2 into the reaction chamber. What happens to the forward reaction rate right after the injection of the N2? What happens to the reverse reaction rate right after the injection of the N2? What happens to the forward reaction rate after the injection of the N2 until equilibrium is re-established? What happens to the reverse reaction rate after the after the injection of the N2until equilibrium is re-established? When equilibrium is established, what is the relationship between the forward and the reverse reaction rate?

Question

The chemical reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) is at equilibrium. An experimenter injects a small amount of N2 into the reaction chamber. What happens to the forward reaction rate right after the injection of the N2? What happens to the reverse reaction rate right after the injection of the N2? What happens to the forward reaction rate after the injection of the N2 until equilibrium is re-established? What happens to the reverse reaction rate after the after the injection of the N2until equilibrium is re-established? When equilibrium is established, what is the relationship between the forward and the reverse reaction rate?

Answer 1

at injectionk, forward increases, reverse remains same, until equilibrium it increases in the forward, after injection, the reverse starts to increase as the products are increased, at equilibrium the rates are equal in both directions.

Answer 2

To answer these questions, we need to understand the concept of Le Chatelier's principle. According to Le Chatelier's principle, when a stress is applied to a system at equilibrium, the system will shift in a way that helps to counteract the stress and restore equilibrium.

1. Right after the injection of N2:
- The forward reaction rate initially increases because there is an increase in the concentration of N2, which leads to more collisions between N2 and H2 molecules, favoring the formation of NH3.
- The reverse reaction rate also increases because there is an increase in the concentration of NH3, which leads to more collisions between NH3 molecules and H2, favoring the reverse reaction.

2. Until equilibrium is re-established:
- As the forward reaction rate increases, more products (NH3) are formed, thus increasing the concentration of NH3.
- The increased concentration of NH3 will cause the reverse reaction rate to gradually increase as the system tries to counteract the stress and restore equilibrium.

3. When equilibrium is re-established:
- The forward and reverse reaction rates become equal, resulting in no net change in the concentrations of the reactants and products over time.
- At equilibrium, the rates of the forward and reverse reactions are equal, which means the system reaches a dynamic balance. The forward and reverse reaction rates are said to be equal or in equilibrium.

In summary, the forward reaction rate initially increases after the injection of N2, as does the reverse reaction rate. However, over time, both rates gradually decrease until reaching equilibrium, where they become equal to establish a balance between the forward and reverse reactions.