## 7th Ed. 7A.15

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

daniella_knight1I
Posts: 57
Joined: Fri Sep 28, 2018 12:18 am

### 7th Ed. 7A.15

I'm having difficulty calculating the order for C. I found A and B, but I keep getting weird numbers for C. Can anyone explain how to figure that one out?

Laura Gong 3H
Posts: 89
Joined: Fri Sep 28, 2018 12:26 am
Been upvoted: 1 time

### Re: 7th Ed. 7A.15

So for C, I think you'll find that your work will get you:
1^z/2^z = 1 where z=the order in relation to reactant C.
This just means that z=0 so the reaction is zero order for reactant C.

Hope this helps!

taline_n
Posts: 64
Joined: Fri Sep 28, 2018 12:17 am

### Re: 7th Ed. 7A.15

To calculate the order for C, I used experiments 1 and 4. I divided experiment 1 ([A]=10^x, [B]=100^y, [C]=700^z) by experiment 4 ([A]=10^x, [B]=100^y, [C]=400^z). The rates for exp 1/exp 4 are 2/2=1 (so your order for C will have to result in a rate of 1). [A] and [B] cancel out, so you're left with 1=1.75^z. This means that in order for 1.75 to become 1, z=0. C is a zeroth order reaction.