equilibrium shit Flashcards
collision theory
how chemical reactions are justified
when is equilibrium achieved, relating to concentrations
Because the activation energy is different for the reactant converting to products than it is for products converting to reactants, the equilibrium will be achieved when the concentrations of products and reactants are different.
equilibrium constant
Ratio of products to reactants
[products]/[reactants]
if Keq is a very large number?
great deal of the product compared to reactant
if Keq is a very small number?
very little product compared to the amount of reactant present at equilibrium.
HOW DOES ONE RECOGNIZE CHEMICAL EQUILIBRIUM
No changes in any measurable or observable (macroscopic) properties
Concentrations (pressures), colours, etc. of the species present in the reaction cease to change
The reaction seems to have stopped
CHEMICAL EQUILIBRIUM
A dynamic state of balance in a chemical reaction where the concentration (or pressures) of all reactants and products remains constant at all the time
the forward rate equals the reverse rate
when products = reactants, what is Keq?
1
products > reactants, what is Keq?
> 1
products < reactants, what is Keq?
< 1
LE CHATELIER PRINCIPLE
Le chatelier discovered that if you take a system at equilibrium and you impose a change upon it, the system will attempt to counteract the change
Impact of pressure on concentration and reaction, overall?
If we increase partial pressure of only one of the gases it is the same as increasing its concentration
this speeds up the reaction.
We can increase the overall pressure by decreasing the volume
If we decrease overall volume, all the pressures go up equally
changes in pressure only affect what kinds of equilibriums?
an equilibrium with unequal number of moles of gaseous reactants and products
impact of increasing the pressure of a gas reaction on equilibrium
shifts the position of equilibrium towards the side with fewer molecules
increasing and decreasing concentration impact on Keq
- Increasing the concentration of reactants causes the formation of more products (right shift!!)
- Decreasing the concentration of reactants causes a pull in the direction of the products (left shift!!)
- Decreasing the concentration of product will cause a right shift!
- Increasing the concentration of product will cause a left shift!!
