## 15.15

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

Jesus Rodriguez 1J
Posts: 53
Joined: Sat Jul 22, 2017 3:00 am

### 15.15

Would the answer to this problem be considered to be a second order because it relies on both of the concentrations or would it be a first order because both concentrations are first order?

Danah Albaaj 1I
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

### Re: 15.15

The reaction would be first order because the reaction rate is increased in direct proportion to each reactant's concentration.

Nhan Nguyen 2F
Posts: 52
Joined: Thu Jul 13, 2017 3:00 am
Been upvoted: 1 time

### Re: 15.15

If you increase or decrease a concentration and its rate of reaction also increases or decreases at the same rate, you have a first order reaction