Contents
content
|
page
|
Abstract
|
2
|
Introduction
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3
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Literature review
|
5
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Objectives
|
7
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Methodology
|
8
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Results
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11
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Discussion
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14
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Conclusion and
recommendation
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15
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Reference
|
16
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Appendix
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17
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Abstract
This is an
experiment to study chemical equilibrium and Le Chatelier’s Principles.
Chemical equilibrium is the stable state a chemical reaction reaches when there
is no further undergoing reaction or change. Le Chatelier’s Principles state
that when a chemical equilibrium is disturbed by certain changes, it will shift
the position of equilibrium towards the side to minimize the effect of the
changes applied.
In this
experiment, six sets of chemical reaction were carried out to study the effect
of adding particles or ions of reactants or products to the position of
equilibrium.
(i)
The saturated sodium chloride solution
equilibrium
(ii)
The iron (III) thiocyanate ion
equilibrium
(iii)
The acetic acid equilibrium
(iv)
The chromate-bichromate equilibrium
(v)
The bismuth chloride-water equilibrium
(vi)
The cobalt (II) chloride equilibrium
The shifting of equilibrium can be determined
from the colour of the solution or mixture since the reactions chosen in this
experiment have reactants of different colours from corresponding products, or
undergo other distinct changes.For example, in the first part of the
experiment, concentrated hydrochloric acid was added to a saturated solution of
sodium chloride. The chloride ions yield by concentrated hydrochloric acid had
increased the chloride ion concentration which is a product of hydration of
sodium chloride. Hence, the changes were observed and shifting of this
equilibrium position was deduced.
This
experiment must be conducted very carefully and the substances must be measured
and added very accurately because any slight error might influent the outcome
of the experiment. Besides, the mixture of substances must be stirred well
until the substances are will mixed and form a mixture of same physical state
(homogeneous solution), in this experiment, liquid.
The
experiment outcome supports Le Chatelier’s Principles in the aspect of
concentration. When the concentration of a particle in an equilibrium is
altered, the equilibrium position will shift to the direction to counteract the
change. In this experiment, the concentrations of product or reactant particles
were increased by adding like particles (the same substance or substance
containing like ions). The equilibriums conducted shifted to the opposite
direction of the increased concentration, and produced more particles of the
substances it shifted to.
