## products in rate law equation

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

Ariana de Souza 4C
Posts: 99
Joined: Wed Sep 21, 2016 2:56 pm

### products in rate law equation

Hey guys
in the course reader on page 60, it says that we're only going to be focusing on initial rates that are a function of only reactant concentration. but in the textbook, on page 621, it says that rate laws may depend on the concentrations of prouctsa s well as those of reactants. It uses O3 --> O2 as an example, and the rate law is k * ([O3]^2/ [O2]).
Should we be concerned about these reactions for the quiz?

Abbas_Hakim_1B
Posts: 18
Joined: Wed Sep 21, 2016 2:57 pm

### Re: products in rate law equation

I don't think so. The course reader also states that the products should also be removed continuously to keep the product concentration low so that it doesn't affect rate equation. Hope this helps!

Riley Seid 1L
Posts: 13
Joined: Wed Sep 21, 2016 2:55 pm

### Re: products in rate law equation

And if we do end up needing those more specific formulas/values, I believe they will be provided, similarly to constants or tabular data.

Cris-1C
Posts: 7
Joined: Mon Jan 26, 2015 2:17 pm

### Re: products in rate law equation

I'm pretty sure that if the course reader does not cover it, then we are not expected to know other than what Lavelle mentions in class. Therefore, since the course reader does say that only reactants will be covered in an an attempt to make the rate laws much simpler, then I believe we need not worry about any diversions involved in the textbook.

Cayla_Brooks_1I
Posts: 10
Joined: Mon Jan 26, 2015 2:17 pm

### Re: products in rate law equation

If we balance a rate law equation and end up with fraction coefficients, is there another way to solve the problem and find the error without plotting/graphing?