Identify the true statement about the rate of the forward and reverse reaction once a reaction has reached equilibrium. (a) The rate of the forward reaction and the reverse reaction is zero. (b) The rate of the forward reaction is greater than the rate of the reverse reaction. (c) The rate of the reverse reaction is greater than the rate of the forward reaction. (d) The rate of the forward reaction is equal to the rate of the reverse reaction.

Video transcript

Hello everyone today. We have The following problem describes what happens to the rate of the reaction when chemical equilibrium is achieved. So, in a state of chemical equilibrium, the reaction is reversible and what reversible just implies that the reaction can proceed forward in the forward direction or the reverse direction. And so the rate of the forward reaction is going to be equal to the rate of the reverse reaction. And eventually the concentration of our reactions and products will reach a constant level. So if we look at our answer choices, we looking at options B and C. And these are simply not true. And so why aren't they true? Well, neither. Well, it's because neither the reverse nor the forward reaction will go at a faster rate. Right? So we're going to say that the rate of our reactant equal the rate of our products. This is what it means to be an equilibrium. So B and C are not correct. If you look at answer choice D. This is not correct either. Because when the rate of the reaction approaches zero, this means that the reaction has ceased to be dynamic and no longer is at equilibrium. And so that leaves and toys A to be the correct one. The rates of the forward and backward reactions or reverse reaction become equal. And with that we've answered the question overall, I hope that this helped. And until next time