## First Order Reactions [ENDORSED]

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

William Lan 2l
Posts: 73
Joined: Fri Sep 29, 2017 7:07 am

### First Order Reactions

When a reaction is first order, does it mean that it's faster or slower than a second order reaction?

Eli Aminpour 2K
Posts: 50
Joined: Fri Sep 29, 2017 7:04 am

### Re: First Order Reactions

It depends on the reaction and the amount of concentration available. Its too general to say all of one is faster than another

Vincent Tse 1K
Posts: 30
Joined: Fri Sep 29, 2017 7:05 am
Been upvoted: 1 time

### Re: First Order Reactions  [ENDORSED]

If a reaction is "first order", it simply means that the rate is proportional to the concentrations of one of the reactants.
If a reaction is "second order", it simply means that the rate is proportional to the SQUARE of the concentrations of that reactant.
A reaction being first order does not necessarily indicate that it is faster than a second order reaction, just that changing the concentrations of a reactant in the first order reaction has a less "drastic" effect on the rate than if you made that same concentration change to a second order reaction.