## 15.3

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

Emily Glaser 1F
Posts: 156
Joined: Thu Jul 27, 2017 3:01 am

### 15.3

Why don't we divide the average rate by the number of moles.

In this problem, when I found reaction rate of NO2, I got 0.0065 mole/Ls

Why wouldn't I divide or multiply that number by 2 based off the equation given of 2NO2 --> 2NO + O2?

Audrey Goodman 1F
Posts: 31
Joined: Fri Sep 29, 2017 7:06 am

### Re: 15.3

The concentrations you are given are in terms of NO2 so there is no need to convert them as we are finding the rate of reaction in terms of NO2. You can see that in part b, you must use the coefficients to find the rate of formation of O2.

504754253
Posts: 45
Joined: Fri Jun 23, 2017 11:39 am

### Re: 15.3

can someone send me lecture notes from 03/02/18 as well as 02/28/18... I had a dentist and doctors appointment these days my email is breaunnecrockett@gmail.com

RohanGupta1G
Posts: 34
Joined: Sat Jul 22, 2017 3:00 am

### Re: 15.3

As someone already said, the units are already Moles of N02 L^-1S^-1 so you don't need to divide by moles of N02

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