How might a compound be zero-order?
Im confused to exactly why a compound might be zero-order in a reaction. Like what makes it have no influence on the rate of reaction? for my experiment I studied potassium permanganate and oxalic acid and found permanganate was a zero-order and had no influence on the rate of reaction. Why might this be? I thought maybe because oxalic is in excess but I'm not too sure. Any help would be good!
- Mike ALv 71 month ago
It usually means that the overall reaction proceeds in multiple steps and you have a rapid first step followed by a much slower step leading to the product(s).
A <====> A* (Rapidly established equilibrium)
A* + B --------------> Products (slow)
The rate will be;- k[A*][B]
But [A*] will be constant until most of the A is used up,
so you can rewrite the rate as:- k'[B] where k' = k[A*]
Other examples can be found here: