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IB Chemistry SL
Equilibrium
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Cards (15)
Many reactions are
reversible
and exists in a state of
equilibrium.
In a dynamic equilibrium, both the
forward
and
reverse
reactions occur at
equal
rates.
At equilibrium, there is no change in the
concentration
of reactants or products.
Homogeneous
equilibrium
All reactants and products are present in
one
phase
Heterogeneous
equilibrium
Reactants and products are present in more than
one
phase
A catalyst increases both the rate of forward and reverse reaction
equally.
Hence, there is
no
effect on the equilibrium position or
K
c
K_c
K
c
Equilibrium constant formula
a
A
+
aA+
a
A
+
b
B
⇌
c
C
+
bB\rightleftharpoons cC+
b
B
⇌
c
C
+
d
D
dD
d
D
K
c
=
K_c=
K
c
=
[
C
]
c
[
D
]
d
[
A
]
a
[
B
]
b
\frac{[C]^c[D]^d}{[A]^a[B]^b}
[
A
]
a
[
B
]
b
[
C
]
c
[
D
]
d
The equilibrium constant is only affected by
temperature.
What affects the equilibrium position?
Change in
concentration
Change in
pressure
(only if in
gaseous
state)
Change in
temperature
Effect of
conditions
on equilibrium
Le Chatelier's principle
If a dynamic equilibrium is
disturbed
, the
equilibrium position
shifts to
counteract
the change and establish a new equilibrium.
If the concentration of a reactant is increased, the
forward
reaction will be favored to counteract this. Vice versa.
K
c
(reverse)
K_{c\text{ (reverse)}}
K
c
(reverse)
=
=
=
1
K
c
(forward)
\frac{1}{K_{c\text{ (forward)}}}
K
c
(forward)
1
A small
K
c
K_c
K
c
value (
K
c
K_c
K
c
<
<
<
1
1
1
) implies that
reactants
are favored over
products
.
A large
K
c
K_c
K
c
value (
K
c
K_c
K
c
>
>
>
1
1
1
) implies that
products
are favored over
reactants.
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