## 15.3/Unique Rate

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

Alexandra Carpenter 1G
Posts: 32
Joined: Sat Jul 22, 2017 3:00 am

### 15.3/Unique Rate

In the problem, the reaction is given as N2(g) --> 3 H2(g) + 2 NH3(g). The unique rate if reaction is half of the rate of reaction for NO2. When finding this, do we divide by the coefficient of the reactant only?

Matthew Lee 3L
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

### Re: 15.3/Unique Rate

Yes, because you are using the reaction rate of the reactant, NO2, you divide by its stoichiometric coefficient, which in this case is 2.

Johann Park 2B
Posts: 51
Joined: Thu Jul 27, 2017 3:01 am
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### Re: 15.3/Unique Rate

Did you mean the reaction: 2NO2 -> 2NO + O2?

Then yes, the decomposition of NO2 is used to find the unique rate of the reaction which is 1/2(Δ[NO2]/Δt)