## How to solve

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

205192823
Posts: 100
Joined: Wed Sep 18, 2019 12:19 am

### How to solve

For all the 0,1,2 order reactions is it all plug and chug?

BeylemZ-1B
Posts: 95
Joined: Thu Jul 25, 2019 12:17 am

### Re: How to solve

I would say so for the most part. The hardest part is discerning whether it is a first, second, or zeroth order reaction. Don't count on just knowing the basic equations for the final though, I would make sure you are well versed in the reaction graphs (section 7B) and how to analyze them.

Matthew Chan 1B
Posts: 111
Joined: Sat Sep 07, 2019 12:16 am

### Re: How to solve

For the most part, it is just plugging in your values and solving. Sometimes you will need to do some intermediate calculations in order to obtain all the necessary values to calculate the desired answer.

Tauhid Islam- 1H
Posts: 64
Joined: Fri Aug 02, 2019 12:15 am

### Re: How to solve

It's also important to know the relationship between whichever manipulation of the initial concentration of a reactant to time is. That relationship will tell you the order of the reaction. From there, the equations are pretty standard. I think the hardest part to figuring out which order the reaction actually is.