## The integrated rate laws

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

Moderators: Chem_Mod, Chem_Admin

Hector Acosta Discussion 1H
Posts: 51
Joined: Fri Sep 29, 2017 7:04 am

### The integrated rate laws

There are so many ways to write the integrated rate law, which one is the best when solving for concentration final?

Dylan Davisson 2B
Posts: 50
Joined: Thu Jul 27, 2017 3:00 am
Been upvoted: 2 times

### Re: The integrated rate laws

The only real reason you see the basic integrated rate laws look so many different ways is because they are being manipulated to answer specific values that the problem gives. All of the variations of the integrated rate laws all have the same basic structure. The typical way of writing the integrated rate law can be seen in Outline 4 : Chemical Kinetics on the class website. I would recommend starting with this basic structure for the equation for the sake of simplicity. You really only need to know the one equation for each of the 3 orders that apply to the class (zero, first, and second).

Shawn Patel 1I
Posts: 54
Joined: Thu Jul 27, 2017 3:01 am

### Re: The integrated rate laws

Hey,
The basic versions of the integrated rate laws for each reaction order is given during the tests. Any different versions of the laws are just algebraic manipulations that you can perform yourself if needed.

Daniisaacson2F
Posts: 30
Joined: Sat Jul 22, 2017 3:00 am

### Re: The integrated rate laws

Just use the integrated rate laws that he gives on the equation sheet!

Return to “First Order Reactions”

### Who is online

Users browsing this forum: No registered users and 1 guest