## Reaction Orders [ENDORSED]

$\frac{d[R]}{dt}=-k[R]; \ln [R]=-kt + \ln [R]_{0}; t_{\frac{1}{2}}=\frac{0.693}{k}$

Hailey Johnson
Posts: 31
Joined: Wed Nov 16, 2016 3:04 am

### Reaction Orders

Can someone help clarify what the different reaction orders mean and how we use them?

Nisarg Shah 1C
Posts: 54
Joined: Sat Jul 22, 2017 3:00 am

### Re: Reaction Orders

Reaction orders are the sum of the order of each reactant. Each reactant's order tells us about how the concentration of that reactant affects the rate of formation of the products. For example, a zero-order reaction means that for a certain reactant, the concentration of it doesn't affect the rate of formation of products. Meanwhile for a second-order reaction, it means that the rate of formation of the product is the square of the concentration of a certain reactant.

Justin Folk 3I
Posts: 43
Joined: Wed Sep 21, 2016 2:56 pm

### Re: Reaction Orders  [ENDORSED]

They basically mean, in crass terms, "How much does the concentration of reactant affect rate of reaction"