Based on their activation energies and energy changes and assuming that all collision factors are the same, rank the following reactions from slowest to fastest. (a) Ea = 45 kJ>mol; E = -25 kJ>mol (b) Ea = 35 kJ>mol; E = -10 kJ>mol (c) Ea = 55 kJ>mol; E = 10 kJ>mol

Video transcript

Hi everyone for this problem we want to answer which of the following reactions will be the fastest. Assume that the collision factors for the reactions are equal. So in order to solve this problem, we're going to need to write out the Iranians equation which is our rate constant is equal to our pre exponential factor times E. Raised to our negative activation energy over R times T. Okay, So we want to know which of the following will be the fastest and were provided with activation energies. So we're comparing activation energy to our rate constant. And here they have an inverse relationship. So that means what happens to one, The opposite will occur to the other. And in the problem specifically asked for which will be the fastest. So that means which one is going to cause our rate constant. K to be the fastest. And because it has an inverse relationship with activation energy, that mean our lowest activation energy is going to have the highest rate constant. And out of all the answer choices given we can see that answer choice C is our lowest activation energy, which means this is going to be our correct answer. 50 kg joules per mole will be the fastest. That's the end of this problem. I hope this was helpful