## Negative Orders

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

nelms6678
Posts: 53
Joined: Fri Sep 29, 2017 7:07 am

### Negative Orders

Can a reaction order be negative? If so, how?

Yashaswi Dis 1K
Posts: 56
Joined: Fri Sep 29, 2017 7:04 am

### Re: Negative Orders

It can because rate law is experimentally determined so if the experiment yields a result that allows for a negative reaction order then that is possible. Typically I don't think we will be dealing much with negative reaction order because it is not as common but it is good to know that it can exist.

Angel R Morales Dis1G
Posts: 50
Joined: Sat Jul 22, 2017 3:01 am

### Re: Negative Orders

A previous post stated that their T.A told them that we should be comfortable with negative orders for the final, but we shouldn't worry about fractions or stuff like that.

Yeyang Zu 2J
Posts: 58
Joined: Fri Sep 29, 2017 7:06 am

### Re: Negative Orders

It can be negative, which means as the substances decreases , the reaction rates increases. Try to think of the relationships between products and forward reaction

Cynthia Bui 2H
Posts: 30
Joined: Fri Sep 29, 2017 7:05 am

### Re: Negative Orders

A reaction can be negative with respect to one reactant but I don't think all reactants can have a negative order. The overall order for a reaction has to be at least 0.

sallina_yehdego 2E
Posts: 75
Joined: Sun Apr 29, 2018 3:00 am

### Re: Negative Orders

Yes, negative orders are possible and just means that whatever the substance is, it decreases and cases the reaction rate to increase. I had the same confusion, but a TA told me to get familiar with negative orders and fractions.