Use the reaction to answer the question.
3MnO₄ ²⁻ + 4H⁺ ⇄ 2MnO₄⁻ + 2H₂O + MnO₂(s)
How would adding MnO₄²⁻ ions affect this reaction?
a) The equilibrium would shift to the right, and the concentration of MnO₄⁻ ions would increase.
b) The equilibrium would shift to the left, and the concentration of H₂O would decrease.
c) The equilibrium would shift to the left, and the concentration of H+ ions would increase.
d) The equilibrium would shift to the right, and the concentration of MnO₂ would decrease.
Adding MnO₄²⁻ ions would shift the equilibrium to the right, and the concentration of MnO₄⁻ ions would increase. Therefore, the correct answer is (a).
Well, adding MnO₄²⁻ ions to the reaction is like inviting more guests to a party. They bring the party vibes with them! So, the equilibrium would shift to the right, meaning option a) is the correct answer. The concentration of MnO₄⁻ ions would increase, making the reaction party even more exciting!
To determine the effect of adding MnO₄²⁻ ions on this reaction, we need to analyze the reaction equation and consider Le Chatelier's principle.
The reaction equation is:
3MnO₄²⁻ + 4H⁺ ⇄ 2MnO₄⁻ + 2H₂O + MnO₂(s)
Adding MnO₄²⁻ ions would increase the concentration of the reactant on the left side of the equation. According to Le Chatelier's principle, an increase in the concentration of a reactant will cause the reaction to shift to the right, towards the products, in order to counteract the increase.
Therefore, the correct answer is:
a) The equilibrium would shift to the right, and the concentration of MnO₄⁻ ions would increase.
To determine how adding MnO₄²⁻ ions would affect the given reaction, we need to consider Le Chatelier's principle. According to this principle, when a stress is applied to a system at equilibrium, the system will respond by shifting in the direction that reduces the stress.
In this case, adding more MnO₄²⁻ ions would increase their concentration, which can be considered a stress to the system. To reduce this stress, the system would shift in the direction that consumes MnO₄²⁻ ions.
From the given balanced equation, we can see that MnO₄²⁻ ions are consumed in the forward reaction to form MnO₄⁻ ions and MnO₂(s). Therefore, adding more MnO₄²⁻ ions would cause the equilibrium to shift to the right (forward reaction), resulting in an increase in the concentration of MnO₄⁻ ions and MnO₂(s).
So, the correct answer is:
a) The equilibrium would shift to the right, and the concentration of MnO₄⁻ ions would increase.