## Difference b/w General Rate Laws/Elementary

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

Joseph Saba
Posts: 154
Joined: Thu Jul 11, 2019 12:16 am

### Difference b/w General Rate Laws/Elementary

Lavelle states on a worksheet on his website that
"2N2O(g) → 2NO(g) + O2(g)
• Write the overall rate expression for this first-order reaction.
rate= k[N2O]
*Note that the exponent does not match the coefficient in front of N2O. By just looking at the overall balanced equation, you cannot tell the order of the reaction."
What's the difference b/w elementary and 1st,2nd,0 order reactions? But in the book when discussing elementary rate laws, they discuss the concept of bimolecular and unimolecular reactions. Can we combine these ideas and say a reaction is unimolecular and 1st order? But if that logic applies, then the example lavelle had would be incorrect? Any clarification would be much appreciated.

Aliya Jain 2B
Posts: 101
Joined: Wed Sep 11, 2019 12:16 am

### Re: Difference b/w General Rate Laws/Elementary

I'm pretty sure we can associate something that is first order with being unimolecular!

PranaviKolla2B
Posts: 114
Joined: Fri Aug 30, 2019 12:17 am

### Re: Difference b/w General Rate Laws/Elementary

Does someone have a good video or link explaining the difference between first order and second order reactions in terms of what is actually happening in the reactions rather than the math associated with either?