Concerning the following reaction at equilibrium:
3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would:
Answer A. Shift the equilibrium to the right
B. Shift the equilibrium to the left
C. No change
D. Increase the value of the equilibrium constant, K
E. Decrease the value of the equilibrium constant, K
Hmm, let me put on my clown nose for this one! 🤡
Well, if we increase the concentration of the Fe(s), it's like saying we're adding more clowns to the circus. And you know what happens when you add more clowns, right? Chaos! 🎪
So, in this case, increasing the concentration of Fe(s) would disrupt the delicate equilibrium and shift it to the left, trying to restore order to the circus... uh, I mean, the reaction. So, the answer is B - Shift the equilibrium to the left.
Remember, chemistry can be serious, but it's always more fun with a few clown antics thrown in! 🎉
To determine the effect of increasing the concentration of Fe(s) on the equilibrium, we need to consider Le Chatelier's principle. According to this principle, if a stress is applied to a system at equilibrium, the system will adjust to relieve that stress and establish a new equilibrium.
In this reaction, Fe(s) is one of the reactants. Increasing its concentration would be considered a stress on the system. To relieve this stress, the system would want to decrease the concentration of Fe(s). To do so, it will shift the equilibrium towards the right, favoring the forward reaction. Therefore, the answer is A. Shifting the equilibrium to the right.
To determine how increasing the concentration of Fe(s) would affect the equilibrium, let's consider Le Chatelier's principle. According to this principle, when a system at equilibrium is subjected to a change, it will respond in a way that counteracts the change.
In this reaction, the Fe(s) is one of the reactants. Increasing the concentration of Fe(s) means adding more Fe(s) to the system. According to Le Chatelier's principle, the system will respond by trying to decrease the concentration of Fe(s) and reach a new equilibrium.
To do this, the reaction will shift in the direction that consumes more Fe(s). Looking at the balanced equation, we see that Fe(s) is a reactant, so the reaction would shift to the right to consume more Fe(s).
Therefore, increasing the concentration of Fe(s) would shift the equilibrium to the right.
The correct answer is A. Shift the equilibrium to the right.