An Investigation into Electrolysis - Copper Sulphate

An Investigation into Electrolysis - Copper Sulphate

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An Investigation into Electrolysis - Copper Sulphate

Introduction


Decomposition caused by electricity is called electrolysis. The
electrical energy causes a chemical change. When a salt is dissolved
in water, its ions become free to move so the solution can be
"electrolyzed." The products of the electrolysis depend on the
chemical solution, its strength and the type of electrode. The cathode
is negatively charged and therefore attracts to it positive ions. E.g.
hydrogen. The more reactive substance stays in the solution whereas
the less reactive is released and appears as a gas (hydrogen) or a
coating of metal. At the anode (positively charged) the negative
charges are given up; for example chlorine or oxygen ions become
elements.

Electrolysis is used to produce gases or purify metals.

PLAN

Aim: To find out if the current being transferred through copper
sulphate affects the amount of copper transferred.

Prediction: I predict that as the amount of electrical current is
passed through the copper sulphate solution more copper will be
transferred. I also predict that the rise in electrical current and
the rise in copper transferred will be related, and follow a trend.
e.g.

Text Box: Copper Transferred[IMAGE]

I believe that as the current doubles so will the amount of copper
transferred.

E.g. 1amp = 0.1 gram of copper transferred - 2amps = 0.2 grams of
copper transferred.

I think this will happen because it is logical that when something is
doubled the affected will be doubled as well. Also to back up my
theory is Faraday's Law:

Faraday's First Law of electrolysis states that:

"The mass of any element deposited during electrolysis is directly
proportional to the number of coulombs of electricity passed"

Faraday's Second Law of electrolysis states that:

"The mass of an element deposited by one Faraday of electricity is
equal to the atomic mass in grams of the element divided by the number
of electrons required to discharge one ion of the element."

Research:

I have researched other possible ways to work out a rough idea of what

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Related Searches

the results may be:

Charge (C) = Current (A) x Time (sec.)

· Moles of Electrons or Faradays = Charge (C) / 96500

· Moles of Copper = Moles of electrons or Faradays / ratio=2

· Mass = moles x RAM

· If the Current is 0.2A and the time taken 5 minutes

· Charge = 0.2 x (5x60)

· Faradays = 60/96500

· Moles of Copper = 0.0006217/2

· Mass = 0.0003108 x 64

· Mass = 0.0199 grams

· If the Current is 0.2A and the time taken 10 minutes

· Charge = 0.2 x (10 x 60)

· Faradays = 120/96500

· Moles Copper = 0.0012435/2

· Mass = 0.0006217 x 64

· Mass = 0.0398 grams

· If the current is 0.2A and the time taken 15 minutes

· Charge = 0.2 x (15 x 60)

· Faradays = 180/96500

· Moles Copper = 0.0018652/2

· Mass = 0.0009326 x 64

· Mass = 0.0597 grams

· If the current is 0.2A and the time taken 20 minutes

· Charge = 0.2 x (20 x 60)

· Faradays = 240/96500

· Moles Copper = 0.002487/2

· Mass = 0.0012435 x 64

· Mass = 0.0759 grams

· If the current is 0.2A and the time taken 25 minutes

· Charge = 0.2 x (25 x 60)

· Faradays = 300/96500

· Moles Copper = 0.0031088/2

· Mass = 0.0015544 x 64

· Mass = 0.0995 grams

Apparatus: Ammeter, power pack, 2x copper plates, copper sulphate,
beaker, electrical wires, scales.

Measurements:
I am going to measure, by weighing, the weight of both the copper
anode before and after each change in current. I will weigh the
electrode to the nearest 100th of a gram to give me accurate results
on which to base my conclusion. I am measuring the weight of one
electrode only as I believe it would take to long, and would be a
pointless exercise to weigh both. I would expect the weight of the
anode to decrease with increased current. The change in mass of copper
indicates reaction rate so that the more copper deposited at the
cathode, the faster the reaction rate. I will need to ensure that the
anode is washed, dried and re-weighed after each test to ensure a fair
test.

Method:

1. Set up the apparatus -

2.

* Put copper sulphate solution into the beaker.

* Weigh the anodes original weight and make note of this.

* Clip the copper plates to the sides of the beaker, making sure
they are in the copper sulphate solution.

* Connect the power pack and ammeter to the copper plates,
creating a circuit.

* Adjust the ammeter to display the correct readings.

* Switch on the power pack and adjust the current.

* Leave the current to pass through the copper sulphate for 5
minutes and weight the anode, again making note of this.

* Repeat the last stage.


Safety: Copper sulphate is an irritant so I will be careful not to get
it on my hands or eyes. Goggles will be worn to prevent it going in my
eyes.
----------------------------------------------------------------------

Fair test:
In order to carry out a fair test, the only variable to be changed
will be the current (amount of electricity) passing through the copper
sulphate solution.

The experiment carried out aimed to monitor the quantity of Copper
(Cu) metal deposited during the electrolysis of Copper Sulphate
solution (CuSo4) using Copper electrodes, when certain variables were
changed. It was considered that the following factors could affect the
deposition of Copper metal on the cathode.

1. Time

2. Current

3. Temperature

4. Concentration of Solution

5. Quantity of Solution

6. Size of Electrodes

7. Distance between the electrodes

8. The surface of the electrodes

I will ensure the following variables are kept constant:

· Concentration and amount of copper sulphate solution.

· Voltage.

· Time - Each test will run for 5 minutes.

· Temperature - The experiment will take place at room temperature.

Reliability: To ensure that the results are reliable and accurate I
will perform the test at each temperature twice and take the average.
I didn't perform the test more that twice because it would have taken
to long and I believe that performing the experiment twice will
provide accurate and reliable results.

Obtaining Evidence

I used a wide range of equipment and materials to obtain the evidence
required for this experiment. I managed their surrounding environment
to ensure that I obtained accurate results.

I decided to conduct the obtaining of the evidence in the following
way:

1. Once the experiment had been set up correctly (see apparatus in
the plan section) I made sure that all the equipment was working
correctly. I did this by doing a "trail" experiment (see "trial"
in "plan" section).

2. I conducted the "true" experiment, and recorded measurements
given.

3. I repeated the "true" experiment again and recorded the second
set of measurements for the anomalous results.

4. I displayed the results in a table and a graph.

Results:

Start Weight (g)

Amps (A)

Finish Weight (g)

Weight Loss (g)

1.100

0.2

1.08

0.02

1.08

0.4

1.04

0.04

1.04

0.6

0.995

0.06

0.995

0.8

0.95

0.09

0.95

1.0

0.005

0.10

This was my only anomalous result; it was quite a small, the result
should have been as below. I put both the anomalous result onto the
graph.

0.995

0.8

0.915

0.08

(GRAPH)

Analysing & Considering Evidence

The results obtained support the prediction that the longer the
current is left to flow, the more Copper metal is deposited on the
cathode. It is now true to say that if the time is doubled the charge
is doubled, and therefore the amount of copper produced. Proof of this
can be seen in the obtained results.

Conclusion: I conclude that the results obtained support the
prediction that the longer the current is left to flow, the more
Copper metal is deposited on the cathode. It is now true to say that
if the time is doubled the charge is doubled, and therefore the amount
of copper produced.

The actual results produce an almost straight-line graph, showing
that:

The mass of Copper is relative to the Time the current flows.

Therefore, it has now been proved, through this experiment, that both
of Faraday's Laws Of Electrolysis are correct.

Faraday's First Law of electrolysis states that:

"The mass of any element deposited during electrolysis is directly
proportional to the number of coulombs of electricity passed"

Faraday's Second Law of electrolysis states that:

"The mass of an element deposited by one Faraday of electricity is
equal to the atomic mass in grams of the element divided by the number
of electrons required to discharge one ion of the element."

It has also been discovered that the copper anode releases copper ions
and electrons, which form copper at the cathode.

Evaluation

Although this was a successful experiment, there were some factors of
the experiment, which could have been improved to make it even more
successful. One of these factors could have been the electrodes,
which, even after a good clean were still quite dirty and obviously
still had irremovable substances from previous experiments still
attached to them. If this experiment were to be repeated for a second
time, in need of greater accuracy, it would be imperative to have a
new pair of electrodes, which have never been used before.

Another factor which may have affected the overall outcome of the
investigation may have been the fact that the practical work of the
investigation was carried over from lesson to lesson, meaning that
variables such as the concentration or the amount of the Copper
Sulphate solution could have changed between lessons. To overcome this
problem, a stock solution of Copper Sulphate should have been made so
as the concentration remained the same at all times. The same
electrodes and equipment should have been used throughout. Also, when
weighing, the same electrical balance should have been used as there
may have been slight differences between the two balances. This is
what could explain the anomaly in the graph.
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