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2286215
Equilibria
Description
Mind Map on Equilibria, created by Amy Holden on 16/03/2015.
No tags specified
aqa
a level chemistry
equilibria
chapter 2
Mind Map by
Amy Holden
, updated more than 1 year ago
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Created by
Amy Holden
over 9 years ago
16
2
0
Resource summary
Equilibria
Many reactions are reversible
Eg. alcohol + carboxylic acid <--> ester + water
For any reaction that reaches an equilibrium
aA + bB + cC <--> xX + yY + zZ
Kc = ([X]^x [Y]^y [Z]^z) / ([A]^a [B]^b [C]^c)
Kc = equilibrium constant
This varies for different reactions
The units change depending on the reactants
[X] = concentration of X
units = mol dm^-3
x = the number of moles of substance X
Kc = [products] / [reactants]
Dynamic Equilibrium = the rate of the forwards reaction is equal to the reverse reaction
When doing calculations using the equilibrium constant expressions, make sure you divide everything by the volume of the system
The volumes may cancel
Endothermic reactions (positive∆H)
Decrease of temperature
causes Kc to decrease
causes the products to decrease
causes the reactants to increase
the equilibrium moves left
Increase of temperature
causes Kc to increase
causes the products to increase
causes the reactants to decrease
the equilibrium moves right
Exothermic reactions (negative ∆H)
Increase of temperature
causes Kc to decrease
causes the products to decrease
causes the reactants to increase
the equilibrium moves left
Decrease of temperature
causes Kc to increase
causes the products to increase
causes the reactants to decrease
the equilibrium moves right
Catalysts
They have no effect on the position of the equilibrium
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