chemical equilibrium Flashcards
occurs when a
reaction and its reverse reaction proceed at
the same rate
chemical equilibrium
approaching equilibrium vs equilibrium
pag nag aapproach, both forward and reverse ang nag ooccur
pag equilibrium na, same rate na
what happens to the amount of reactants and products at equilibrium
each remains constant
Forward reaction:
N2O4 (g) → 2 NO2 (g)
- Rate law:
Rate = kf [NO2]2
Reverse reaction:
2 NO2 (g) → N2O4 (g)
- Rate law:
Rate = kr [N2O4]
Keq =
Kf / Kr
ratio products to reactants
the value of k is affected by
substances in g or aq phase (s and l has no effect on position/shift of equilibrium)
catalyst
speeds up forward and reverse reaction, it does no shift equilibrium
noble gases
no effect on equilibrium
types of chemical equilibrium
homo (g) (g) → (g)
hetero (g) (s) → (g)
what does the value of k mean
k»_space; 1 product favored
k «_space;1 reactant favored
manipulating equilibrium constants
coefficients multiplied to n = ^n
reverse = reciprocal
Q
not for equilibrium
Q AND K
Q = K equilibrium
Q > K shifts left (too much product)
Q < K shifts right (too much reactant)
increase in pressure
decrease volume shift
to less moles
what happens to k when temp increases in exothermic reaction?
decreases
if changes in temperature cause the reaction to shift right
k increases
