Electrolysis
of WaterProblem:
How can you perform
Electrolysis of water to produce Hydrogen and Oxygen?
Research the Problem:
Electrolisis is Chemical change, especially
decomposition, produced in an electrolyte by an electric
current. Electrolytes dissolve by dissociation. That is when the
molecules of the substance break down into charged particles
called ions. An ion with a negative charge is called an anion
because it is drawn through the solution to the positive charge
on the anode. A particle with a positive charge is called a
cation. It moves through the solution to the cathode. Water has
its solvent properties because it is polar. The molecule has
charged ends (+ and -). These charged ends react with charges on
other polar substances to dissolve them. They do so by taking
hydrogen atoms from the substance to form hydronium ions. The
word electrolysis means the process of breaking molecules to
smaller components by using an electric current. Positive and
negative poles of a DC electric source such as a battery can
absorb opposite ions of an electrolyte causing separation of
ions and creation of a new substance.
Hypothesis: Adding some Sulfuric Acid as electrolyte
will increase conductivity of water and creation of Hydrogen and
Oxigen gases.
Experiment:
In this experiment, initially we used two copper wires,
one twelve-volt battery, and some drinking water to do the
tests. The process was slow and caused excessive amounts of
corrosion on the copper wires and discoloration in the water. To
avoid corrosion of electrodes and discoloration of water, we
repeated the test using Graphit Rods as electrodes. Also to
speed up the process we added some Sulfuric Acid to the water as
electrolyte.
Materials Used:
Copper Wire, Graphite Rods, Sulfuric Acid, Test Tubes,
Beaker, Water
Procedure:
Fillup ¼ of beaker with clear watter, secure two test
tubes filled with water in the beaker in a way that test tubes
are up-side down over the beaker. Mount the wires or electrodes
that you have prepared and then connect the electricity.
Check the
produced hydrogen and oxygen gasses in five minutes. Repeat the
test with different electrodes and different amounts of
electrolytes and record the results in the table below. You may
want to repeat the experiment with different electrods. (Electrod
is only the area that has contact with water, not the part that
has insulator or plastic cover. In the above picture electrodes
are identified with yellow color).
| Electrode |
No
Additive |
5%
Salt |
5%
Sulfuric Acid |
10%
Sulfuric Acid |
| Aluminum |
|
|
|
|
| Steel |
|
|
|
|
| Platinum |
|
|
|
|
| Copper |
|
|
|
|
| Graphite |
|
|
|
|
Now, Analyze
your data and come up with your own conclusion.
|
