Equilibrai Flashcards
What is dynamic equilibrium
It occurs in a closed system the rate of forward reaction and backward reaction at constant rate and there is constant concentration of products and reactants
How does reaction go ahead and the rate of reaction
At the start there are may reactants but not many products so the reactants collide through successful collisions and form products overtones there is an increase of products so it’s harder for the reactant to come into contact with each other so decrease rate of reaction
Overtime there will be a backward reaction which form reactants again then become constant
What is pe chanteliers principle
If a change is applied to dynamic equilibrium the equilibrium position shifts to position to oppose the change
What is the equilibrium constant
If the equation is equal at constant temp
What affects or doesn’t affect equilibrium constant
Equilibrium constant is affected by temperature and not affected by concentration or pressure or with a catalyst
How does a change of pressure affect equilibrium position and change in concentration
There are more particles in a set volume so more crowded enviroment so there will be more reaction in order to oppose the change equilibrium position moves to side with the lowest miles to oppose the increase of the pressure
How does a change in temperature affect the equilibrium constant
It affects how the forward reaction and affects the backward reaction at different extents so affect the equilibrium constant
How does temp change equilibrium position
The rate of reaction increase as the particles have more kinetic energy so collide more often and frequently increasing rate of reaction however if the forward reaction is exothermic the equilibrium position will move to the left to oppose the increase to f the temperature so decreases the yield you get to equilibrium faster but smaller yield
How does a catalyst affect equilibrium
Doesn’t affect position of equilibrium as affects forward and backward reaction equally
However it does increase the rate of reaction as it provides activation energy which is lower more particles have required activation energy so more collisions lead to more successful collisions so reach equilibrium at a faster rate
