I found this question in the AP Chem book, and I understand why B is the answer (as the answer key says). However, I don't understand why D is not also correct.
The question is:
A multistep reaction takes place with the following elementary steps.
- Step I. A + B <-> C
- Step II. C + A -> D
- Step III. C + D -> B + E
Why would increasing the temperature make the reaction rate go up?
- (A) it is an endothermic reaction that needs an outside energy source to function
- (B) The various molecules in the reactions will move faster and collide more often
- (C) The overall activation energy of the rxn will be lowered
- (D) A higher fraction of molecules will have the same activation energy
I understand that B is correct based on collision theory, but why isn't D correct as well? Don't a greater % of molecules have the same activation energy at higher temperatures? (Or am I misinterpreting answer choice D?)