Lecture 11-14 (Ch.15): Equilibrium, Equilibrium Constant, ICE Table, Reaction Quotient(Q), Le Chatelier's Principle Flashcards
dynamic equilibrium
- forward and reverse rxn rates are equal
- have diff. conc. of chemicals but conc. are constant
equilibrium constant (K)
- ratio of chemical concentrations at equilibrium
- has NO units
- only consider gas and aqueous phases(not solids/liquids)
why is the size of K important
- indicates more prdts or rxts at equilibrium
- if K is large (>1) products favored
- if K is small (<1) reactants favored
Kp
- equilibrium in terms of pressure
- easier to measure pressure than concentration
- does NOT have a unit
what equation relates Kc to Kp?
Kp=Kc(RT)^Δn
R: 0.08206
-NO units
when manipulating K, what happens when you multiply an equation?
-you raise K to that power
when manipulating K, what happens when you reverse an equation?
-take reciprocal of K
when manipulating K, what happens when you add equations?
-then multiply K’s
when do you use an ICE table?
-when all values are not et at equilibrium and need to determine what equilibrium looks like
equilibrium constant (K)
-ratio of chemical concentrations in a rxn at equilibrium
reaction quotient (Q)
- ratio of chemical concentrations in a rxn not yet at equilibrium
- size of Q related to K indicates the direction the rxn will shift to establish equilibrium
le chatelier’s principle
-add away, take towards
if pressure increases, what side would it shift to?
- shift to side w less gas mols
- volume decreases
- need fewer gas particles to reduce the number of collisions (creating less pressure)
if volume increases, what side would it shift to?
- shift to side w more gas mols
- pressure decreases
if an inert gas is added, what side would it shift to?
-no change bc not in K expression
