## units

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

inlovewithchemistry
Posts: 104
Joined: Fri Sep 28, 2018 12:19 am

### units

are the common units for k values (mol/L*s) and the units for overall reactions (L/mol*s)? why are these different in textbook problems?
Last edited by inlovewithchemistry on Mon Mar 11, 2019 7:28 pm, edited 1 time in total.

LorenzoDuvergne3I
Posts: 60
Joined: Fri Sep 28, 2018 12:25 am

### Re: units

I don't think they really carry any significance other than showing that your end units are always going to be mol/L/s, and k's units are going to be designed to cancel out any units for the other terms so that your end result is mol/L/s.

sophiebillings1E
Posts: 60
Joined: Fri Sep 28, 2018 12:27 am

### Re: units

There's no real units for k it's based off what the problem entails whether given concentration or partial pressure.