## 15.3

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

Meachelle_Lum_1I
Posts: 92
Joined: Fri Sep 28, 2018 12:24 am

### 15.3

For 15.3 part a when finding the reaction rate of NO2, how come we don't divide by 2, the coefficient of NO2?

Posts: 60
Joined: Tue Nov 28, 2017 3:02 am

### Re: 15.3

Reaction rate depends on the duration of the NO2 not the coefficient of the substance. It would be the change in concentration over the time duration of a reaction thus it would be divided by 20s instead of 2.

Kate_Santoso_4F
Posts: 72
Joined: Fri Sep 28, 2018 12:29 am

### Re: 15.3

The rate of reaction of NO2 can be found by the change in concentration of NO2 divided by the change in time. We are given the initial and final concentrations of NO2 in the problem (450 mmol/L to 320 mmol/L) and the change in time (20s). Therefore, the rate of reaction of NO2 is -(320 mmol/L - 450 mmol/L)/20s = 6.5 mmol/L*s or 6.5*10^-3 mol/L*s.

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