## Half life first order reaction rate

$\frac{d[R]}{dt}=-k[R]; \ln [R]=-kt + \ln [R]_{0}; t_{\frac{1}{2}}=\frac{0.693}{k}$

Moderators: Chem_Mod, Chem_Admin

madisondesilva1c
Posts: 91
Joined: Fri Sep 28, 2018 12:16 am

### Half life first order reaction rate

In lecture, we finished by going over how the 1st order reaction rate can appear as a exponential if you take the exponentiate the rate equation for half life. Does this pattern still apply for second order reactions in a similar manner, since exponential is decreasing as a function of initial concentration of reactant, how should we understand behavior in various higher order cases?

Cole Elsner 2J
Posts: 88
Joined: Fri Sep 28, 2018 12:25 am

### Re: Half life first order reaction rate

We haven't really been taught this yet. We JUST finished our first order work, so we should wait for Dr. Lavelle to actually cover this in lecture.

Return to “First Order Reactions”

### Who is online

Users browsing this forum: No registered users and 3 guests