Equilibrium (5/9)
No description yet. This curated deck is ready for daily study.
Card preview (20)
Equilibrium
Forward rate= reverse rat reactant and product concentrations are stable
Non-spontaneous reaction
reaction favors reactant
Keq
Equilibrium constant [products]/[reactants]
The Haber Process
N2 + 3H2 –> 2NH3 Kf[Reactants]=Kr[Products]
Keq when favoring a side has a…
value >1 for products value <1 for reactants
What states of matter does Keq include?
gases
Facts about Keq
Non concentration dependent catalysts change kinetics but not equilibrium
Keq expression for reverse
Keq=[reactants]/[products] or 1/Keq forward -inverse relationship
Reaction quotient
Concentrations can be from any point in reaction, not just equilibrium
Q>Keq
too many products
Q
Too many reactants
La Chatelier principle
When changing concentration of one reactant, the other one may compensate. So, changing concentrations will not change Keq, just change the math that gets us the Keq
When removing product…
It will increase the yield because the reaction is working harder to replenish the product
ASA Synthesis
Add excess reactants or take away the product
Relationship of pressure and volume in Le Chat principle
Increasing volume= decrease pressure and vise versa
Temperature in Le Chat principle
Endothermic= +∆H Exothermic= -∆H
What does heat do regarding equilibrium
R + Heat –> P for endothermic reactions R –> P + Heat for exothermic reactions
Catalyst
Don’t impact thermodynamics and do not effect concentrations at equilibrium. Simply speed up reaction
If volume is increased…
The reaction will shift to the side with more moles
If pressure is decreased…
The reaction will shift towards the side with more moles of gas