## Homework Problem 15.3

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

Mike Matthews 1D
Posts: 59
Joined: Fri Sep 29, 2017 7:04 am

### Homework Problem 15.3

Homework question 15.3: "In 20 s the concentration of nitrogen dioxide, NO2, decreases from 450 mmol.L-1 to 320 mmol.L-1 in the reaction 2NO2(g)--->2NO(g) + O2(g). Determine the rate of reaction of NO2" Why is it that in the answer key the rate of reaction of NO2 is not divided by its stoichiometric coefficient of 2?

Julia Campbell 2F
Posts: 31
Joined: Sat Jul 22, 2017 3:00 am

### Re: Homework Problem 15.3

I think because the product also has a coefficient of two so it's a 1:1 ratio. Or maybe the concentrations given already factored that in.

Lena Nguyen 2H
Posts: 51
Joined: Fri Sep 29, 2017 7:06 am
Been upvoted: 1 time

### Re: Homework Problem 15.3

The question asks for the rate of reaction of NO2 rather than the unique average rate of the reaction (which would divide the rate by 2). Therefore, the rate of reaction of NO2 is the change in NO2 over the change in time multiplied by -1.

sofiakavanaugh
Posts: 58
Joined: Thu Jul 13, 2017 3:00 am
Been upvoted: 1 time

### Re: Homework Problem 15.3

I am also confused on this: if this is true then what exactly is the difference between rate of reaction and unique rate of reaction and why are they calculated differently?

Kailey Brodeur 1J
Posts: 34
Joined: Thu Jul 27, 2017 3:00 am

### Re: Homework Problem 15.3

The rate of reactions cannot be generally inferred from the the chemical equation for the reaction. So the stoichiometric coefficients are the only thing to consider.

### Who is online

Users browsing this forum: No registered users and 2 guests