Equilibrium I & II Flashcards
What happens when reactants get used up in a reversible reaction?
The forward reaction slows down.
What happens when more product is formed in a reversible reaction?
The reverse reaction speeds up.
What is dynamic equilibrium?
This is when the concentration of reactants and products stay constant.
The rate of the forward reaction is the same as the rate of the backward reaction.
Where does a dynamic equilibrium happen?
In a closed system.
Kc tells you what?
How far to the left or right the equilibrium is.
What is an homogeneous system?
This is a system where everything is in the same physical state.
Whay does Kc calculation involve.
The concentration of products over reactants in square brackets to the power of moles for each substance.
What is a heterogeneous system?
This is a system where not everything is in the same state.
What is not included in the heterogeneous Kc? Why?
Solids and pure solid. Their concentration stay constant throughout the reaction.
What does catalyst do to the equilibrium constant?
They speed up the rate at which the dynamic equilibrium is reached.
What is Le Chatelier’s Principle?
It states that when a system in dynamic equilibrium is subjected to a change in conditions the equilibrium position shifts to counteract that change.
How does increasing concentration of a reactant affect equilibrium?
If you increase the concentration of a reactant, the equilibrium shifts to the right,making more product to get rid of the extra reactant.
How does increasing concentration of a product affect equilibrium?
Equilibrium shifts to the left to remove the extra product,this makes the reverse reaction go faster.
What happens to equilibrium position when you increase the pressure?
It shifts equilibrium to the side with fewer gas molecules. This reduces the pressure.
What happens to equilibrium position when you decrease the pressure?
It shifts the equilibrium to the side with more gas molecules.This raises the pressure again.
Describe an exothermic reaction
the reaction releases heat,ΔH is negative, so the forward reaction is exothermic.
Describe an endothermic reaction.
If ΔH is positive, the reaction absorbs heat, so the forward reaction is endothermic.
What happens when you increase the temperature of an exothermic reaction?
