15.17

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

Katelyn 2E
Posts: 35
Joined: Sat Jul 22, 2017 3:01 am

15.17

I'm a little confused as to how [C] is independent of the rate, as stated in the solutions manual.

Alvin Tran 2E
Posts: 39
Joined: Fri Sep 29, 2017 7:06 am

Re: 15.17

The rate doesn't depend on the concentration of C, which means it is independent, because the reaction is zero order with respect to C. If you compare experiments 1 and 4 (where the concentrations of A and B stay the same), the initial concentration of C changes but the initial rate doesn't change.

Eli Aminpour 2K
Posts: 50
Joined: Fri Sep 29, 2017 7:04 am

Re: 15.17

compare the reaction rates when all other reactants remain constant except for C. The reaction rate doesn't change even though C does, meaning it isn't in the rate law because it is a zero order reactant.

Ammarah 2H
Posts: 30
Joined: Fri Sep 29, 2017 7:06 am

Re: 15.17

If you write the rate law, [C] will be to the zero power, meaning that [C] will always be equal to one, meaning it does not change the rate (so it is independent of the rate).

RohanGupta1G
Posts: 34
Joined: Sat Jul 22, 2017 3:00 am

Re: 15.17

As the others said, C is zero order because looking at experiments 1 and 4, even though the concentration of C changes, the initial rate remains the same. This means C has no impact and therefore its exponent is 0.