A reaction proceeds via a two-step mechanism. The first step is a fast, reversible equilibrium with a small equilibrium constant. The second step is slow. Which of the following is MOST likely true about the overall reaction rate?
The overall rate will be determined solely by the rate of the slow step.
The overall rate will be independent of the concentration of the intermediate.
The overall rate will be dependent on the concentrations of the reactants in both steps.
The equilibrium constant of the first step will have no effect on the overall rate.
Related Questions
Two molecules A and B collide, but no reaction occurs. Which of the following MUST be true?
The molecules did not collide with the correct orientation.
The molecules are not reactive under any conditions.
The collision did not have sufficient energy to overcome the activation energy barrier.
The temperature of the system is too low for any reaction to occur.
A reaction proceeds via a two-step mechanism. The first step is a fast, reversible equilibrium with a small equilibrium constant. The second step is slow. Which of the following is MOST likely true about the overall reaction rate?
The overall rate will be determined solely by the rate of the slow step.
The overall rate will be independent of the concentration of the intermediate.
The overall rate will be dependent on the concentrations of the reactants in both steps.
The equilibrium constant of the first step will have no effect on the overall rate.
Which statement is not correct?
For endothermic reactions, heat of reaction is lesser than energy of activation
For exothermic reactions, heat of reaction is more than energy of activation
For exothermic reactions energy of activation is less in forward reaction than in backward reaction
For endothermic reactions energy of activation is more in forward reaction than in backward reaction
