SCH4U h5+, Chemistry, 12, University ­ Virtual High School Unit Assignment: Le Chatelier's Principle and Equilibrium Lab Assignment Request the complete assignment now.

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SCH4U h5, Chemistry, 12, University Virtual High School
Le Chatelier's Principle and Equilibrium Lab Assignment
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Experiment
Le Chatelier's Principle and Equilibrium Lab
Assignment
In this lab activity, you will explore how stress
applied to a variety of
systems at equilibrium will affect the direction in
which the system
will shift to reestablish equilibrium.
Access the virtual lab through the following link:
Equilibrium and Le Chatelier's Principle Virtual
Lab
Equilibrium Equation
When you click on an equilibrium system, the
equilibrium equation is
given above the image.
1)Cobalt System:
The reaction is an exothermic reaction, i.e heat is released when the
reaction happens in the forward direction until the equilibrium is attained.
When heat is added to the system, the reaction shifts in the backward
direction which can be explained applying Le Chatlier’s principle, which
states, if a system at equilibrium is subjected to a stress, the equilibrium is
shifted in the direction that tends to relieve the stress.
The heat is added to a system which is in equilibrium, this is the stress being
applied to the system. In order to relieve the stress the reaction has to be
shifted towards left, causing endothermic reaction, which absorbs the
added heat energy and attains the equilibrium again.
Similiarly when the system is cooled, the Le Chatlier principle states that the
reaction has to be shifted in the forward direction and release some heat
through the exothermic reaction to re-establish equilibrium.
Adding reactants in the reaction causes the reaction to shift in the forward
direction as Le-Chatlier’s principle states that the system proceeds in a
direction to release the added stress. Here the added reactants are
converted to products and the equilibrium is regained. This causes the
solution to turn into red color when water is added.

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Images
The initial image is of the original solution before
the stress has been applied.
Once the stress has been applied, the image on
the left is the original solution and the image on
the right represents how the system reacts to the
stress applied.
Icons
Click on the following icons to apply stress to the
equilibrium system:
Bunsen burner Heating
Beaker with ice Cooling
Flask Adding Chemical Entity
Similarly when the products are added to the equilibrium, the reaction
shifts in the backward direction, converting products to reactants to regain
the equilibrium. This could be observed when potassium chloride is added
to the system, which generates chlorine anion and causes the reaction to
shift in the left direction. This causes the solution to change into blue.
When silver nitrate is added to the solution, it will ionize into silver cation,
and nitrate anion. Silver will react with chlorine to form silver chloride, a
precipitate. Because some of the product is lost, the system will shift to the
right to form the products. Hence the system will change color to red.
2)Iron Thiocyanate System:
Forward reaction is an exothermic reaction, hence when the heat is added
the system shifts in the backward direction to relieve the stress by
absorbing the added heat through the endothermic reaction. Hence the
solution turns pale yellow.
Adding KSCN causes production of SCN- ions, which is a reactant, as
discussed in above application according to Le Chatlier’s principle the
reaction is shifted in forward direction and the solution turns red.
When iron nitrate is added, iron being one of the reactants, again the
reaction is forced in the forward direction and the equilibrium is attained.
The system will turn red.

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Equilibrium Systems
The following equilibrium systems are to be
tested in this lab activity:
Cobalt
Ammonium
Iron thiocyanate
Chromate
Nitrogen Dioxide
Copper Sulfate
Procedure:
1. For each equilibrium system to be tested,
create a data table that includes a column for
predictions, one for observations, and one for
chemical entity formed. Write out the
equilibrium equation at the top of each table.
2. For each stress (heat, cold, chemical) to be
applied to the equilibrium system, predict what
observable change (i.e. color change, precipitate,
etc.) is expected and in which
direction the system will shift to reestablish
equilibrium.
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3. Once you have made a prediction for each
stressor, click on the available icons and record
your observations
Analysis:
For each equilibrium system tested, use Le
Châtelier's principle to provide a brief
explanation of your observations.
Questions:
1. All cells of the body need oxygen.
Haemoglobin is an oxygen transporting
protein that functions to provide oxygen to our
cells. The haemoglobin oxygen complex is an
example of an equilibrium system. The
equilibrium
expression is given below:
Hb(aq) + 4 O2(g)↔ Hb(O2)4(aq)
a. In which direction will the equilibrium shift in
the lungs where there is a high concentration
of oxygen?
b. How does this differ from the concentration
of oxygen in cells in the rest
of the body and in which direction will the
system shift? Why?
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2. The carbonic acidbicarbonate chemical
buffering systems helps to maintain blood pH
and is a good example of Le Châtelier's principle
at work in the human body. The equilibrium
equation is given below:
H+(aq) + HCO3-(aq) ↔ H2CO3(aq) H2O(l) +
CO2(g)
a. Hyperventilating reduces the concentration of
CO2 in the blood and results in dizziness. In
which direction will the equilibrium shift in
response?
b. How would you treat someone who is
hyperventilating? Why?
c. Normal blood pH is between 7.35 and 7.45.
Prolonged, excessive vomiting can lead to
dehydration and an increase in blood pH a
condition known as alkalosis. The kidneys
respond by removing HCO3- (aq)from the blood.
In which direction will the system shift? How
does this restore blood pH to within a normal
range?
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