## 6th edition 15.13

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

davidbakalov_lec2_2L
Posts: 61
Joined: Fri Sep 28, 2018 12:23 am

### 6th edition 15.13

I am having trouble on this problem, how do you do it?

404975170
Posts: 68
Joined: Thu Jul 27, 2017 3:00 am

### Re: 6th edition 15.13

In the solutions manual they make it more difficult to see the different steps involved since they combine it all but all you have to do for part (a) is
convert H2 and I2 to moles and then convert them to a molar concentration by dividing the number of moles obtained for each by the volume 0.750 L.
Then you plug these molarities into the rate law: rate=k[H2][I2]
k=0.063/mol*s

Then for part b since both [H2] and [I2] are first order if you doubled the concentration by 2 it would just multiply the whole rate by 2. rate=k*2[H2][I2]