# Order

Notes on order, this is difficult you may have to read it a few times

- Created by: Mark Freeman
- Created on: 21-06-11 13:11

First 263 words of the document:

Order

Orders are all about concentration, concentration affects reactions because

it caused there to be more collisions per second. Therefore, the reaction is

faster.

The order is how far concentration affects the rate of reaction of a

substance. A substance with a higher order is more affected by a change in

concentration.

For example an order of 0(zero order) means rate is proportional to [C]0

In other words, the rate of reaction does not change when concentration

changes.

But if the order is 2(second order) rate is proportional to [C]2

In other words if the concentration doubles the rate will quadruple (times

by 4), because 4 is 2 squared.

The Rate Equation

The rate equation allows you to identify a relationship between the rate,

the concentrations, and their orders

Rate = k * [A]0[B]1[C]2

This is the rate equation, firstly you probably want to know what k

represents, k represents a constant that is used to get from the

concentrations and orders to the rate.

You work out k like so, k = rate / Concentration

You also have to know how to calculate the overall order, just add upp all

the orders in the equation!

[A]1[B]2 Overall order = 1+2 = 3

K

K has alot of different units, different for each order but luckily you only

need to know four.

Order Unit

0 Moles per decimetre cubed per

second

1 Seconds-1

2 Decimetres cubed per mole per

second

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