## Rate of Reaction

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

Vanessa Romero-Campos 2B
Posts: 39
Joined: Fri Sep 25, 2015 3:00 am

### Rate of Reaction

Can someone explain why -d[NO2]/dt=d[NO]/dt=2 d[O2]/dt
I'm confused about the 2 before the d[O2]/dt
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Jessica Patzlaff 1A
Posts: 28
Joined: Fri Sep 29, 2017 7:05 am

### Re: Rate of Reaction

In the chemical equation, the stoichiometric coefficients show that for every mol of O2 formed there are 2 mol of NO and NO2, so it O2 is forming half as fast. Thus, its rate would have to be doubled to equal the rate of NO being formed and NO2 being broken down.

Timothy Kim 1B
Posts: 62
Joined: Fri Sep 29, 2017 7:04 am

### Re: Rate of Reaction

The 2 is there due to the ratio of the coefficients between the reactants and the products.

AnuPanneerselvam1H
Posts: 52
Joined: Fri Sep 29, 2017 7:07 am

### Re: Rate of Reaction

Since the stoichiometric coefficients are 2 for NO2 and 1 for O2, the rate of O2 production will be half of that of NO2 depletion.

Kayla Tchorz-Dis 1F
Posts: 30
Joined: Thu Jul 13, 2017 3:00 am

### Re: Rate of Reaction

you just need to pay attention to the coefficients, and since o2 is half, theres half as much made