Topic 3- equilibrium Flashcards
describe equilibrium
as system approaches equilibrium, both forward and reverse reactions are occuring
at equal, the forward and reverse reactions are proceeding at the same time
-ones achieved, it will remain constant
when a chemical system at equilibrium is disturbed, what occurs
it will shift to favour the side needed to re reach equilibrium
-overall it will increase both sides
to increase or decrease pressure, what way will the reaction shift
Inc: shifts towards side with fewer mols
dec: shifts to side with more mols
if we have a reaction at equilibrium and then we add gas, will the equilibrium be affected?
-no
-there won’t be an effect
for exothermic reactions (on product side/ neg H), to add heat and remove heat what will way will it shift
add: left
remove: right
or endothermic reactions (on reactant side, pos H ), to add heat and remove heat what will way will it shift
add: right
remove: left
what do we use to achieve equilibrium faster and remains unaltered
a catalyst
K eq formula
kf (products)/ kr (reactants)
-reverse would be reac/products
-ratio becomes exponent
Kc formula
[C]c[D]d / [A]a[B]b
Kp formula for gaseous reactions
Kp= Kc (RT) ^n
-RT is 0.08314
- ^n= prod-reac
-if n= 0 then kp equals kc
are equilibrium answers unitless
yes
if K is»_space;>1 (bigger) or if K«<1 (smaller), which side is favoured
bigger: product favoured
smaller: reactant favoured
Keq formula for multiple steps
Keq=Ksp x Ka x Kb
what is excluded in equilibrium equations
liquids and solids
Kp formula when given partial pressures
=[Prod]exp
______________
P reac x P reac
why is Q quotient used
-We don’t know if the system is at equilibrium and want to check.
-We want to predict how the reaction will shift to reach equilibrium.
Q formula
prod/reactants
determining the shift for Q quotents
more K then Q- goes forward (prod)
K=Q then equilibrium
Less K then Q then reverse reaction (reac)
what do you do when there is liquids and solids only on one side
put it over 1
