Studied by 2 people
Dynamic equilibrium
A closed system with equal rate and concentration of forward and reverse reactions.
Closed system
matter and energy can’t be lost or gained
Open system
Matter and energy can escape
Effect of pressure on equilibrium
increase = equilibrium shifts to side with less volume/number of molecules
Effect of concentration on equilibrium
increase = forward reaction is favored
Effects of temperature on equilibrium
increase = endothermic reaction is favored
only factor effecting Kc
effect of Catalyst on equilibrium
Increase rate of both reactions
No effect on equilibrium
Kc > 1
concentration of product is greater
What factor effects Kc?
Temperature
What happens to Kc if you reverse the equation?
It becomes the reciprocal
What is Q?
Ratio of products and reactants for a reaction that hasn’t reached equilibrium
What is the relationship between Q and Kc at equilibrium?
Q=Kc
What happens if Q>Kc?
The reverse reaction is favored
What happens if Q<Kc?
The forward reaction is favored
Le Chatelier principle
If a change is made to a system at dynamic equilibrium, the position of the equilibrium moves to minimise this change
What happens to Kc when reaction coefficients are doubled?
Kc is squared
What happens to Kc when reaction coefficients are halved?
Kc is square rooted
What happens to Kc if 2 reactions are added?
The Kc values are multiplied
Note 
Flashcard (210)