Eventually, the forward and reverse reaction rates become identical, kf=kr, and the system has reached chemical equilibrium. If the forward and reverse reactions occur at different rates, then the system is not at equilibrium.
This is the main definition of Equilibrium. If at some point k_1 = k_2 that's the point of equilibrium. If that doesn't happen there's no equilibrium to find.
Figure 1.8.3:
I still don't think I fully understand this, but it's a bit easier to think about after doing the Kinetics Discussion worksheet.
If possible, can someone explain this in other words?
If the initial concentration of butadiene is 0.0200 M, what is the concentration remaining after 20.0 min? Answer
Where's the rest of this question? It's giving the initial concentration and the time, where's the third one I need to solve the problem? I need either the [A] or the rate to do the question.
The following table lists kinetics data for this reaction at 25°C. Determine the rate law and calculate the rate constant. kinetics data for this reaction at 25°C. Experiment [S2O82−]0 (M) [I−]0 (M) Initial Rate (M/s) 1 0.27 0.38 2.05 2 0.40 0.38 3.06 3 0.40 0.22 1.76 Answer: rate = k[S2O82−][I−]; k = 20 M−1·s−1
Maybe I missed it, but I didn't see anywhere in this chapter in an example or in word where it tells you what to do when the math for determining the rate doesn't give you a clean integer.
Based on the answer it seems like you can round but I don't get how that makes sense . . . ?