Answer:
See below for detailed answers to each part of the question.
Explanation:
To solve this problem, we must consider Le Chatelier's Principle, which states the equilibrium position of a system will shift to counteract any changes that occur in the system. This principle can be used to answer each part of your question.
In Part i, we know that N2 is a reactant. Decreasing the concentration of N2 would cause this reaction to shift towards the reactants (to the left), effectively producing more N2 to counteract the change. This would simultaneously decrease the concentration of NH3, since this is a product of the reaction.
Considering the next part, also using Le Chatelier's principle, increasing the pressure would encourage the reaction to shift to decrease the pressure. In order to decrease the pressure, the equilibrium should shift to the side with fewer gas molecules. In this case, there are 4 gas molecules in the reactants and 2 in the products, so the equilibrium position shifts to the products (to the right) to decrease the pressure. This would also increase the amount of NH3, since NH3 is a product.
In Part iii, the temperature is increased. To counteract this change, the reaction will shift to decrease the temperature. Since we know that this reaction is exothermic, the equilibrium will shift towards the reactants (left) to decrease the temperature. This would decrease the amount of NH3.
Finally, in Part IV, if a catalyst is added, this will not change the equilibrium position. Catalysts do not change the overall energy change of a reaction, only the activation energy, so no equilibrium shift will be observed. Thus, the amount of NH3 will not increase/decrease but will remain the same.
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