## Rate law equations

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Anika_Patel_1G
Posts: 32
Joined: Fri Sep 29, 2017 7:06 am

### Rate law equations

What is the difference between the equations Rate=k x [concentration]^a and (-1/a)*(d[A]/dt)?

Lourick Bustamante 1B
Posts: 50
Joined: Wed Nov 16, 2016 3:02 am

### Re: Rate law equations

The two equations are equal to each other; therefore, you can use either one. The equation k[R]^n is just the other reaction rate equation reexpressed after doing experiments to observe d[R]/dt. The equation k[R]^n is in terms of the rate constant, k, the concentration of reactant, [R], and the order of reactant, n.

Wenxin Fan 1J
Posts: 53
Joined: Thu Jul 13, 2017 3:00 am

### Re: Rate law equations

They are the same. They are only written using different variables but they ultimately represent the same thing.

Emma Li 2C
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am
Been upvoted: 1 time

### Re: Rate law equations

I think the second one is described as the unique instantaneous rate of a reaction, and the first one as the rate law but they should calculate the same thing!