Order

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

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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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Decimetres 6
per mole squared per
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