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?

When N2 is injected the forward reaction increases because N2 is larger. The reverse direction also increases since products are forming at a greater rate. At the end when equilibrium is re-established the forward reaction rate = reverse reaction rate.

When a small amount of N2 is injected into the reaction chamber, several things occur:

1. Forward Reaction Rate: Initially, the forward reaction rate will increase. This is because the concentration of N2 has increased due to the injection, leading to more collisions between N2 and H2 molecules, resulting in an increased rate of formation of NH3.

2. Reverse Reaction Rate: The reverse reaction rate will also increase initially. This is because the addition of N2 causes an increase in the concentration of NH3, and according to Le Chatelier's principle, an increase in the concentration of a product will favor the reverse reaction. Therefore, more collisions between NH3 molecules will occur, leading to an increased rate of conversion back to N2 and H2.

As the system tries to re-establish equilibrium, the rates of the forward and reverse reactions will change:

3. Forward Reaction Rate until Equilibrium: As more N2 is injected, the concentration of N2 will become higher than the original equilibrium concentration. This will result in an increase in the forward reaction rate initially. However, as the concentration of NH3 increases, the reverse reaction rate will also increase, eventually reaching a point where the forward and reverse reaction rates become equal, signifying the re-establishment of equilibrium.

4. Reverse Reaction Rate until Equilibrium: Similarly, the reverse reaction rate will increase initially due to the increase in NH3 concentration caused by the injection of N2. Eventually, the forward reaction rate will also increase until both rates are equal, indicating the attainment of equilibrium.

5. Equilibrium Relationship: At equilibrium, the forward and reverse reaction rates become equal. This means that the rate at which NH3 is formed from N2 and H2 is equal to the rate at which NH3 is converted back to N2 and H2. The concentrations of all species involved in the equilibrium reaction remain constant, despite the ongoing reversibility of the reaction.

It's important to note that the rates of the forward and reverse reactions depend not only on the concentrations of the reactants and products but also on various factors such as temperature, pressure, and presence of a catalyst, which can affect the equilibrium position and the kinetics of the reaction.