Equilibrium Conditions
Read Pgs 278-286
Pg 287
#1, 2, 3, 5, 7
Answers #1 a) Irreversible, since it is impossible to return the egg to the
raw state.
b) Irreversible, since the dissolved metal cannot become solid again.
c) Reversible, since there is the simultaneous presence of salt in its
aqueous form and its solid form
d) Reversible, since the CO2(g) dissolved in the champagne and the gaseous
carbon dioxide that occupies the space between the champagne and the cork are
constantly changing from one to the other.
#2 a) Open
b) Closed
c) Closed
d) Closed, if bottle is closed.
e) Open
f) Open
#3 Since this system is open, it does not allow the simultaneous presence
of reactants and products. In fact, the constant supply of oxygen continuously
favours the forward reaction. Moreover, since the product molecules are the gas
phase, they dissipate rapidly in the air and their dissapearance also favours
the forward reaction.
#5 a) This system is not in a state of equilibrium, since it is an open
system.
b) This system is in a state of equilibrium. It is solubility
equilibrium.
c) This system is not in a state of equilibrium, since it is not a closed
system. In fact, in this particular case, this system is in a stationary state:
the water entering the system is equivalent to the water leaving the
system.
d) This system is in a state of equilibrium. It is phase
equilibrium.
e) This system is in a state of equilibrium. It is chemical
equilibrium.
#7 a) The solution is not oversaturated with copper sulfate since the
reactants are completely dissolved. The simultaneous absence of reactants and
products prevents the system from attaining equilibrium. While this reaction is
reversible in theory, the experimental conditions do not allow for equilibrium
to be attained and therefore, the reaction can be considered irreversible or
complete.
b) -Decrease the temperature of the system, since a decrease in temperature
generally reduces the solubility of compounds in water.
-Decrease the quantity of water (the volume of the system)
-Increase the initial quantity of the reactants (copper sulfate)
Equilibrium Constant and Conditions
Pg 318
#1, 9, 10
Answers #1a) Kc = [CO][H2O]/[CO2][H2]
b)Kc = [CO2]2/[CO]2
c)Kc =
[NO2][O2]/[NO][O3]
d)Kc = [O2]/[H2O]2
e)Kc = [O2]
#9.a) Complete reaction
b) No reaction.
c) Complete reaction
#10. There is a very slim possibility that the hydrogen and chlorine
will form, and the equilibrium constant is very high, which means that there is
a very large majority of products in the reaction at
equilibrium.
Pg. 298 #1, 2 for Question 2b) the question should read: "the pressure of
the system is decreased by increasing its volume?" 6, 7
Answers
#1 a) A: The forward reaction (toward the products) will be favoured.
B: The reverse reaction (toward the reactants) will be favoured.
C: The forward reaction (toward the products) will be favoured.
D: The reverse reaction (toward the reactants) will be favoured.
b) A: No reaction will be favoured.
B: The forward reaction (toward the products) will be favoured.
C: No reaction will be favoured.
D: The reverse reaction (toward the reactants) will be favoured.
c) A: The forward reaction (toward the products) will be favoured.
B: The forward reaction (toward the products) will be favoured.
C: The forward reaction (toward the products) will be favoured.
D: The reverse reaction (toward the reactants) will be favoured.
#2 a) The reverse reaction (toward the reactants) will be favoured.
b) The reverse reaction (toward the reactants) will be favoured.
c) The forward reaction (toward the products) will be favoured.
d) No reaction will be favoured since the addition of a catalyst does not
shift the state of
equilibrium.
#6 Will post in class
#7 -Add HCl
-Add oxygen
-Remove Chlorine as it is produced
-Remove water vapour
-Increase temperature
-Increase pressure on the reaction system
Pg. 304 #1, 2, 5, 6
Answers
#1 a) Graph B b) Graph A c) Graph C
#2 a) The reverse reaction (toward the reactants) will be favoured.
b) No reaction will be favoured since carbon is a solid.
c) The forward reaction (toward the products) will be favoured.
d) The reverse reaction (toward the reactants) will be favoured.
e) The reverse reaction (toward the reactants) will be favoured.
f) No reaction will be favoured.
g) The forward reaction (toward the products) will be favoured.
h) The reverse reaction (toward the reactants) will be favoured.
i) The forward reaction (toward the products) will be favoured.
#5 a) False. The rate of formation of the products is equsal to that of the
reverse reaction, that is, the formation of the reactants.
b) False. Although the concentration of the reactants or the concentration
of the products no longer vary they are not necessarily equal.
c) True. This system cannot be in a state of equilibrium since it contains
only one compound whose physical state does not change.
d) False. In the case of reactions occurring in an aqueous solution and
that do not emit any gas, there is almost no exchange of matter between the
system and the environment, and the system is considered closed even if it is
not closed physically.
e) False. In the case of the dissolution reaction of a compound in solid
state, the solution must be saturated or supersaturated with this compound in
order for the system to attain a state of equilibrium.
f) False. The system must also be closed and the reaction that occurs must
be reversible. Moreover, aside from temperature, all of the macroscopic
properties of the system must be constant.
#6 Global warming could jeopardize the survival of this species sicne it
could disrupt the equilibrium between male and female newborns. A generalized
increase in the temperature of the planet could result in the birth of more male
alligators than females, which, in the long term, could lead to the extinction
of this species.
Pg. 318 #12
Answers
#12 The temperature should be kept as low as possible.
Read Pgs 278-286
Pg 287
#1, 2, 3, 5, 7
Answers #1 a) Irreversible, since it is impossible to return the egg to the
raw state.
b) Irreversible, since the dissolved metal cannot become solid again.
c) Reversible, since there is the simultaneous presence of salt in its
aqueous form and its solid form
d) Reversible, since the CO2(g) dissolved in the champagne and the gaseous
carbon dioxide that occupies the space between the champagne and the cork are
constantly changing from one to the other.
#2 a) Open
b) Closed
c) Closed
d) Closed, if bottle is closed.
e) Open
f) Open
#3 Since this system is open, it does not allow the simultaneous presence
of reactants and products. In fact, the constant supply of oxygen continuously
favours the forward reaction. Moreover, since the product molecules are the gas
phase, they dissipate rapidly in the air and their dissapearance also favours
the forward reaction.
#5 a) This system is not in a state of equilibrium, since it is an open
system.
b) This system is in a state of equilibrium. It is solubility
equilibrium.
c) This system is not in a state of equilibrium, since it is not a closed
system. In fact, in this particular case, this system is in a stationary state:
the water entering the system is equivalent to the water leaving the
system.
d) This system is in a state of equilibrium. It is phase
equilibrium.
e) This system is in a state of equilibrium. It is chemical
equilibrium.
#7 a) The solution is not oversaturated with copper sulfate since the
reactants are completely dissolved. The simultaneous absence of reactants and
products prevents the system from attaining equilibrium. While this reaction is
reversible in theory, the experimental conditions do not allow for equilibrium
to be attained and therefore, the reaction can be considered irreversible or
complete.
b) -Decrease the temperature of the system, since a decrease in temperature
generally reduces the solubility of compounds in water.
-Decrease the quantity of water (the volume of the system)
-Increase the initial quantity of the reactants (copper sulfate)
Equilibrium Constant and Conditions
Pg 318
#1, 9, 10
Answers #1a) Kc = [CO][H2O]/[CO2][H2]
b)Kc = [CO2]2/[CO]2
c)Kc =
[NO2][O2]/[NO][O3]
d)Kc = [O2]/[H2O]2
e)Kc = [O2]
#9.a) Complete reaction
b) No reaction.
c) Complete reaction
#10. There is a very slim possibility that the hydrogen and chlorine
will form, and the equilibrium constant is very high, which means that there is
a very large majority of products in the reaction at
equilibrium.
Pg. 298 #1, 2 for Question 2b) the question should read: "the pressure of
the system is decreased by increasing its volume?" 6, 7
Answers
#1 a) A: The forward reaction (toward the products) will be favoured.
B: The reverse reaction (toward the reactants) will be favoured.
C: The forward reaction (toward the products) will be favoured.
D: The reverse reaction (toward the reactants) will be favoured.
b) A: No reaction will be favoured.
B: The forward reaction (toward the products) will be favoured.
C: No reaction will be favoured.
D: The reverse reaction (toward the reactants) will be favoured.
c) A: The forward reaction (toward the products) will be favoured.
B: The forward reaction (toward the products) will be favoured.
C: The forward reaction (toward the products) will be favoured.
D: The reverse reaction (toward the reactants) will be favoured.
#2 a) The reverse reaction (toward the reactants) will be favoured.
b) The reverse reaction (toward the reactants) will be favoured.
c) The forward reaction (toward the products) will be favoured.
d) No reaction will be favoured since the addition of a catalyst does not
shift the state of
equilibrium.
#6 Will post in class
#7 -Add HCl
-Add oxygen
-Remove Chlorine as it is produced
-Remove water vapour
-Increase temperature
-Increase pressure on the reaction system
Pg. 304 #1, 2, 5, 6
Answers
#1 a) Graph B b) Graph A c) Graph C
#2 a) The reverse reaction (toward the reactants) will be favoured.
b) No reaction will be favoured since carbon is a solid.
c) The forward reaction (toward the products) will be favoured.
d) The reverse reaction (toward the reactants) will be favoured.
e) The reverse reaction (toward the reactants) will be favoured.
f) No reaction will be favoured.
g) The forward reaction (toward the products) will be favoured.
h) The reverse reaction (toward the reactants) will be favoured.
i) The forward reaction (toward the products) will be favoured.
#5 a) False. The rate of formation of the products is equsal to that of the
reverse reaction, that is, the formation of the reactants.
b) False. Although the concentration of the reactants or the concentration
of the products no longer vary they are not necessarily equal.
c) True. This system cannot be in a state of equilibrium since it contains
only one compound whose physical state does not change.
d) False. In the case of reactions occurring in an aqueous solution and
that do not emit any gas, there is almost no exchange of matter between the
system and the environment, and the system is considered closed even if it is
not closed physically.
e) False. In the case of the dissolution reaction of a compound in solid
state, the solution must be saturated or supersaturated with this compound in
order for the system to attain a state of equilibrium.
f) False. The system must also be closed and the reaction that occurs must
be reversible. Moreover, aside from temperature, all of the macroscopic
properties of the system must be constant.
#6 Global warming could jeopardize the survival of this species sicne it
could disrupt the equilibrium between male and female newborns. A generalized
increase in the temperature of the planet could result in the birth of more male
alligators than females, which, in the long term, could lead to the extinction
of this species.
Pg. 318 #12
Answers
#12 The temperature should be kept as low as possible.
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