what does dynamic equilibrium mean
the rate of the forward reaction is the same as the rate of the backward reaction in a closed system, and the concentrations of the reactants and products are constant
what does it mena if equlinrium lies to the left/right in relation to prducts and reactants
left - when there is more reactants than products in the equilibrium mixture
right - when there is more products than reactants in the equilibrium mixture
factors affecting position of equilbrium
- concentration of a component
- pressure of a system
- temperature
what does homogenous system mean
homo XD
- all reactants nad products are in the same phase
what does heterogenous system mean
at least 2 different phases are present
what does a phase mean
- like state but allows liquids that are immersible to be different phases
what doe s alarge Kc value mean
the qeuilibrium lies to the right
Kc=
- [prodcuts]/[reactants]
- constant, same value at same temperature, unaffected by pressure
eg. aA + bB —> cC + dD
so Kc = [C]^c x [D]^d/[A]^a x [B]^b
what is Q
ask a teacher perchance xx
mathematical realtionship between concentrations of components in a reaction
q=kc
what does a small Kc means <1
equilibrium lies to the left
how to calculate Kc
i - initial moles
c - change in moles
e - equilibrium moles
c - concnetration at equlibrium (eq moles/volume)
substitute the concnetrations into the [products]/[reactants] equation
what is le chatelier’s prinicple
if a change is made to a system in dynamic equilibrium, the position of the equilibrium moves to counteract this change
how does changing temp affect the equilbrium and affect on Kc
- if we increase temperature the equlibrium will shift to the endothermic direction
- if the backwards reaction was endothermic, the denominator of Kc increases therefore Kc decreases
- if the forwards reaction was enfothermic, the numerator of Kc would increase therefore Kc increases
how does changing pressure affect the equilbrium
An increase in pressure will cause the equilibrium to move towards the side with the fewest molecules.
A decrease in pressure will cause the equilibrium to move towards the side with the most molecules.
how does changing concentration affect the equilbrium and Kc
- equilibrium will move towards the products in order to use up the extra reactant added
- rate of the reaction temporarily increases and the system is no longer in equilibrium
- Kc doesn’t change
- if you incrrease concnetration of product number of Q increase so equlibrium shifts left to increase denominator and restore Q=Kc
Kp =
(p Products)/(p Reactants)
partial pressure =
mole fraction x total pressure
what is mole fraction
moles of individual gas/moles of all gas
how does temperature affect Kp
- favours endothermic side
- denominator of Kp Increase thereofre Kp decreases
how does change in partial pressure of one gas affect Kp
-ie. change in conc of one gas
- Kp doesn’t change
eg one reactnat increases:
- denominator of Q increases
- equilibrium shifts rigth tot restor Q=Kc
how does change in total pressure affect Kp
equlibrum shifts ot side with fewest moles
lowkey is there anythign else for Kp xx
tell me !! (wonder girls refrence what >.<)
