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Bvt. Maj. Gen. Joshua Lawrence Chamberlain
is by far the easiest factor to analyze: if our reactants are concentrated, they will collide more often. Higher number of collisions means higher possibility to react. Higher possibility to react means higher velocity of reaction.
So simple!
I have to note that, of course, when reactants start consuming, their concentration lowers, and so the velocity of the reaction lowers as well. So simple (x2)!
aren’t much more difficult, either. Imagine a gold mine, where only one miner can work. As soon as the miner finds his fair amount of gold, he will run to the bank, leaving the place for another one to step in. There is no room for both to work simultaneously, so the speed of the process which depletes of gold our mine is limited by the speed of one working miner.
On the other hand, if we had room for ten or twenty miners, our mine would be salvaged in reasonably less time, with as many workers working simultaneously!
The same applies for our reactions: if the reactants can “touch” each other over small surfaces (interface between immiscible liquids, solids with big particle sizes, etc), they will react much more slowly than they would if they could share wider surfaces.
on the other hand, works in a really smooth and simple way. We know that there is a relationship between kinetic energy and temperature (Eq. 1.50 on page 1-35 of the Physical chemistry textbook): for this reason, it is easy to state that higher temperatures mean higher kinetic energies.
This has two effects:
Because of their utter importance, catalysts deserve a post on their own, so stay tuned for Part III.
I leave you with the thought that in little deeds, an explanation abides!
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