## Rate Law

$K = \frac{k_{forward}}{k_{reverse}}$

TeaK1C
Posts: 17
Joined: Fri Sep 25, 2015 3:00 am

### Rate Law

In the course reader the equation: NO2 + CO --> NO + CO2 has a rate law of: k[NO2]^2
Why does the rate law have NO2 going to the power of 2 when NO2 doesn't have a coefficient of 2?

Ashlee Joan Macalino 3J
Posts: 36
Joined: Fri Sep 25, 2015 3:00 am

### Re: Rate Law

The superscript "n" is indicative of the order of the reaction, not necessarily correlating to the coefficients of a given concentration of products or reactants. Here's a helpful video I found discussing the rate of orders of reaction and what it has to do with concentrations: https://www.khanacademy.org/science/chemistry/chem-kinetics/reaction-rates/v/rate-law-and-reaction-order