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chemistry
equilibrium
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system
the
chemical
reaction
surroundings
everything
external
to the
system
(e.g.
temp
)
open system
matter
+
energy
exchanged
w
surroundings
closed system
only
energy
exchanged
w
system
reversible
products
react
again to
reform
original
reactants
(
BOTH
DIRECTIONS) [⇌]
• e.g. most chem reactions, changing
state
irreversible
products
can't
reform
original
reactants
(
ONE
DIRECTION)
• e.g. baking cake, combustion
rate vs time graph
• [
reactants
] ↓ , [
products
] ↑
•
products
collide to reform
reactants
• eventually,
forward
and
reverse
reactions proceed at
same
rate → at
EQUILIBRIUM
• [
reactants
] + [
products
] remain
constant
concentration - time
graph
•
products
always start at
0M
• ↑ [
products
], ↓ [reactants]
• plateau =
EQUILIBRIUM
•
change
is based on the
mole
ratio
dynamic state
forward
+
reverse
reactions occur
concurrently
at
same
time
(not ceased)
rate of reaction
change
in
concentration
of
reactant
or
product
over time (
M/s
)
extent
of reaction
how far
forward
reaction proceeds
before
EQUILIBRIUM
• not related to ROR
• concentration of R + P are diff for diff equilibrium mixture
equilibrium yield
the
amount
of
products
present at
EQUILIBRIUM
relative to the
amount
of
reactants
4
properties for equilibrium
1. must occur in
closed
system
2. rate of
forward
+
reverse
reactions are
equal
3.
temperature
+
pressure
are
constant
4. [
products
] and [
reactants
] are
constant
equilibrium law
K = [
PRODUCTS
]/ [
REACTANTS
]
only in
homogenous
chem systems
units: P coeff - R coeff
explaining equilibrium law
Q < K → net
forward
reaction (right)
Q = K → system at
EQUILIBRIUM
Q > K → net
reverse
reaction (left)
equation reversed
K
inverted
(reciprocal)
equation doubled
K
squared
equation halved
K
square
rooted
value of K : extent of reaction : relative concentration at equilibrium
less than 10^-4 :
negligible
: ↑ [
reactants
], ↓ [
products
]
b/w 10^-4 and 10^4 :
significant
:
significant
[reactants] and [products]
greater than 10^4 :
almost complete
: ↓ [
reactants
], ↑ [
products
]
greater or equal to 10^5 :
complete
: all
reactants
converted
to products
effect of change in temperature on
endothermic
reactions
• energy
ABSORBED
from surroundings
• favoured by ↑ in
temp
• ↑ temp = ↑
K
(
F
)
• ↓ temp = ↓
K
(
R
)
effect of change in temperature on
exothermic
reactions
• energy
RELEASED
into
surroundings
• favoured by ↓ in
temp
• ↑ temp = ↓
K
( R )
• ↓ temp = ↑
K
( F )
Le
Chatelier's
Principle
states “if a system at equilibrium is subjected to a change, the system will adjust itself to
partially
oppose
the
effect
of the
change”
effect of position on equilibrium:
temperature
+
EXOthermic
reactions
• this is an
exothermic
reaction
•
exothermic
reactions are favoured by ↓ T → act to
release
energy into surroundings
• ↓T (↓ energy in the surroundings) → causes net
forward
reaction to release energy (↑ K)
• ↑T (↑ energy in the surroundings) → causes net
reverse
reaction to absorb energy (↓ K)
effect of position on equilibrium:
temperature
+
ENDOthermic
reactions
• this is an
endothermic
reaction
•
endothermic
reactions are favoured by ↑ T → act to
absorb
energy from surroundings
• ↑T (↑ energy in the surroundings) → causes net
forward
reaction to absorb energy (↑ K)
• ↓T (↓ energy in the surroundings) → causes net
reverse
reaction to release energy (↓ K)
effect of position on equilibrium:
DILUTING
solution
by
doubling
volume
of water
• diluting solution by doubling volume of water = ↓ concentration of all species by
1/2
• LCP states the system will act to partially oppose the change by ↑
concentration
of the system
• moves to side w
most
particles
• net _____ reaction (depends on reaction)
effect of position on equilibrium:
DOUBLING
VOLUME
of container with a gaseous system
• doubling volume of container = ↓ pressure of system by
1/2
• ↓ concentration all species by 1/2
• LCP states the system will act to partially oppose the change by ↑
pressure
of the system
• moves to side w
most
particles
• net _____ reaction (depends on reaction)
effect of position on equilibrium:
HALVING
VOLUME
of container with a gaseous system
• halving volume of container = ↑ pressure of system by
double
• ↑ concentration all species by
double
• LCP states the system will act to partially oppose the change by ↓
pressure
of the system
• moves to side w
least
particles
• net _____ reaction (depends on reaction)
effect of position on equilibrium:
adding a
CATALYST
• catalysts ↓
Ea
of forward + reverse reactions equally
• ↑
rate
of forward + reverse reactions equally
•
no
change in [products] and [catalyst] or K or yield of products
•
no
effect on
position
of equilibrium
effect of position on equilibrium:
adding an
INERT
GAS
• inert gas ↑ total
pressure
of system
• however, doesn’t change
partial
pressure
of
reactants
+
products
•
no
change in [products] and [reactant] or K or yield of products
•
no
effect on
position
of equilibrium
effect on position at equilibrium:
adding
reactants
• adding reactant = ↑ concentration of
reactant
• sharp ↑ in concentration of
reactant
(on graph)
• LCP states the system will act to
partially oppose
the change by ↓ concentration of
reactant
•
net
forward
reaction
effect on position at equilibrium:
removing
products
• removing products = ↓
concentration
of product
•
sharp
↓ in
concentration
of reactant (on graph)
• LCP states the system will act to
partially
oppose
the change by ↑
concentration
of product
•
net
forward
reaction
effect on position at equilibrium:
adding
product
• adding product = ↑
concentration
of product
•
sharp
↑ in
concentration
of product (on graph)
•
LCP
states the system will act to partially
oppose
the change by ↓
concentration
of product
•
net reverse
reaction
how to increase
yield
• ↑ temp for
ENDOthermic
, ↓ temp for
EXOthermic
• ↑ [
reactants
]
• ↓ [
products
] - sell
• ↑ pressure →
less
particles on product side
• ↓
pressure
→
more
particles on product side
how to increase
ROR
• ↑
temp
- $ + danger
• ↓
volume
= ↑ pressure of gas - $ + danger
• ↑
concentration
• ↑
SA
of solid
• add
catalyst
- $ + reuse
yield
theoretical
: products
expected
if reactants
fully
react
(
stoichem
)
actual yield
: mass of products
actually
obtained
slow
ROR
reaches
equilibrium
loss
of substances during transfers
% yield = (
actual
/
theoretical
) x 100
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