A+B <-> C+D
You mix some of A and B in a closed container and the reaction begins.
As time passes, what happens to the amounts of A & B?
As time goes on, what will happen to the rate at which A & B turn into C + D?
Was there any C & D present when the reaction first started?
As time passes, what happens to the amounts of C & D in the container?
As time goes on, what happens to the rate at which C & D turn into A & B?
When the reaction reaches equilibrium, which chemicals will be present in the container?
When the reaction reaches equilibrium, what will be true of the reaction rates?
When the reaction reaches equilibrium, what will be true about the amounts of reactants and products?
I will be happy to critique your thinking on this.
In the given reaction, A and B react to form C and D, and it is assumed to be a reversible reaction. Let's break down each question one by one:
1. As time passes, what happens to the amounts of A & B?
As the reaction proceeds, the amounts of A and B will decrease because they are being consumed in the reaction.
2. As time goes on, what will happen to the rate at which A & B turn into C + D?
Initially, the rate of the forward reaction (A+B -> C+D) will be high and the rate of the reverse reaction (C+D -> A+B) will be low. Over time, as the concentrations of A and B decrease, the forward reaction rate will decrease, while the reverse reaction rate will increase.
3. Was there any C & D present when the reaction first started?
No, initially there is no C and D present because the reaction hasn't started yet.
4. As time passes, what happens to the amounts of C & D in the container?
As the reaction proceeds, the amounts of C and D will increase because they are being formed as the reaction progresses.
5. As time goes on, what happens to the rate at which C & D turn into A & B?
Similar to the previous question, initially, the rate of the reverse reaction (C+D -> A+B) will be low. However, as the concentrations of C and D increase over time, the rate of the reverse reaction will increase while the rate of the forward reaction decreases.
6. When the reaction reaches equilibrium, which chemicals will be present in the container?
At equilibrium, both forward and reverse reactions will occur at the same rate. This means that the amounts of A, B, C, and D will no longer change over time, and all four chemicals would be present in the container.
7. When the reaction reaches equilibrium, what will be true of the reaction rates?
At equilibrium, the forward and reverse reaction rates will be equal. This is crucial for the stability of the system, where the amounts of reactants and products no longer change.
8. When the reaction reaches equilibrium, what will be true about the amounts of reactants and products?
At equilibrium, the amounts of reactants (A and B) and products (C and D) will remain constant. The forward and reverse reactions occur simultaneously at the same rate, indicating a balance between the formation and consumption of the substances involved in the reaction.