Given the following exothermic, equilibrium reaction:

3 H2(g) + N2(g) <--> 2NH3(g)

Using Le Chatelier's Principle, which of the following changes would shift the equilibrium toward more production of NH3?

To shift the equilibrium towards the production of NH3, we need to determine which changes will cause the reaction to counteract the disturbance. According to Le Chatelier's Principle, this can be achieved by changing the concentration, pressure, or temperature.

1. Increase the concentration of H2 or N2: This will result in a shift in the equilibrium towards the production of NH3 to counteract the increase. Therefore, increasing the concentration of either H2 or N2 will shift the equilibrium towards more production of NH3.

2. Decrease the concentration of NH3: If the concentration of NH3 is decreased, the reaction will produce more NH3 to counteract the decrease. So, decreasing the concentration of NH3 will shift the equilibrium towards more production of NH3.

3. Increase the pressure: Since the reaction involves only gases, increasing the pressure will favor the side with fewer moles of gas. In this case, there are fewer moles of gas on the NH3 side (2 moles) compared to the reactant side (4 moles). Therefore, increasing the pressure will shift the equilibrium towards more production of NH3.

4. Decrease the pressure: Decreasing the pressure will favor the side with more moles of gas. Since the reactant side has more moles of gas, decreasing the pressure will shift the equilibrium towards more production of NH3.

5. Increase the temperature: An increase in temperature favors the endothermic reaction, which in this case is the reverse reaction. So, increasing the temperature will shift the equilibrium towards the reactant side and reduce the production of NH3.

6. Decrease the temperature: A decrease in temperature favors the exothermic reaction, which in this case is the forward reaction. Therefore, decreasing the temperature will shift the equilibrium towards more production of NH3.

Based on Le Chatelier's Principle, increasing the concentration of H2 or N2, decreasing the concentration of NH3, increasing the pressure, or decreasing the temperature will shift the equilibrium towards more production of NH3.

To determine which changes would shift the equilibrium towards more production of NH3 in the given exothermic reaction:

Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in temperature, pressure, or concentration of reactants/products, the system will shift in a direction that minimizes the effect of that change.

In this case, to shift the equilibrium towards more production of NH3, we need to increase the concentration of NH3 or decrease the concentration of H2 and N2. Here are the possibilities:

1. Increase the concentration of NH3: To do this, we can add more NH3(g) to the reaction mixture. By increasing the concentration of NH3, the equilibrium will shift in the reverse direction (from right to left) to try and reduce the excess NH3. As a result, more H2 and N2 will be consumed to produce more NH3.

2. Decrease the concentration of H2: To achieve this, we can remove some H2(g) from the reaction mixture. By decreasing the concentration of H2, the equilibrium will shift in the forward direction (from left to right) to try and replenish the decreased H2. As a result, more NH3 will be produced.

3. Decrease the concentration of N2: To accomplish this, we can remove some N2(g) from the reaction mixture. By decreasing the concentration of N2, the equilibrium will shift in the forward direction (from left to right) to try and compensate for the reduction in N2. This will result in more NH3 production.

It's important to note that changes in pressure and temperature can also affect the equilibrium, but the given reaction does not indicate a change in pressure or temperature. Therefore, only changes in concentration of reactants/products will affect the equilibrium position in this case.

In summary, to shift the equilibrium towards more production of NH3, you can either increase the concentration of NH3 or decrease the concentration of H2 or N2.

Question text

Given the following exothermic, equilibrium reaction:

3 H2(g) + N2(g) <--> 2NH3(g)

Using Le Chatelier's Principle, which of the following changes would shift the equilibrium toward more production of NH3?
a. Adding a catalyst
b. Adding heat
c. Increasing the volume of the container
d. Removing NH3