Equilibrium Flashcards
Concentration
The larger the concentration of reactants the greater chance of a reaction occurring, because more collisions are occurring
Temperature
Higher temperature, molecules move faster=larger kinetic energy = the collisions will be far more energetic = higher probability that a reaction will occur.
Activation energy
The minimum amount of energy required for a reaction to occur
Collision model
- Reactions occur when molecules collide with one another
- Some collisions are violent enough to break bonds
- Not all collisions result in a reaction
Molecular orientation
The molecules must strike each other at the proper angle and orientation in order for a reaction to occur. If the molecules are not lined up correctly no reaction will occur and the molecules will bounce off of each other
Catalyst
A catalyst is a substance that speeds up a reaction without being consumed. Your body contains many types of catalysts that are key in survival
Carbonic anhydrase
This enzyme is crucial in removing carbon dioxide from your blood to form carbonic acid
Allosteric inhibitor
A molecule that bonds to the enzyme changing its shape, causing the substance to not fit in the active site.
Dynamic chemical equilibrium
State where the rates of the forward and reverse reactions are the same
Law of chemical equilibrium
AKA the law of mass action
aA +bB cC+dD
ABCD- products and reactants
abcd- coefficients
K stands for?
Equilibrium constant
Homogenous equilibria
When all substances are in the same state
All solid
Or
All liquid etc.
Heterogenous equilibria
When all the substances are in a different state
One rule for writing the k equations
Pure solids and pure liquids must be excluded from the equilibrium expression
Le chateliers principle
When a change is imposed on a system at equilibrium, the position of the equilibrium shifts in a direction to reduce the effect of the change
