• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
Page
  1. 1
    1
  2. 2
    2
  3. 3
    3
  4. 4
    4
  5. 5
    5
  6. 6
    6
  7. 7
    7
  8. 8
    8
  9. 9
    9
  10. 10
    10
  11. 11
    11

Electrolysis of Copper Chloride

Extracts from this document...

Introduction

ELECTROLYSIS OF COPPER CHLORIDE INTRODUCTION This investigation is aimed to monitor the quantity of Copper (Cu) metal deposited during the electrolysis of copper chloride solution (CuSo4) using Carbon electrodes, when only a specific variable is changed. The passing of a constant electric current through an aqueous copper chloride solution indicates that the passage of ions through this solution results in the chloride ions moving to the anode while positive copper ions (cations) being discharged at the cathode. This statement is empowered by the ionic theory of electrolysis, which states that the cations are attracted to the cathode and anions towards the anode. At the anode (+): Cl? ions lose an electron to the positive anode and form a neutral chlorine atom. Cl? Cl + e? The chlorine atoms then join up in pairs to form molecules of chlorine gas, Cl2. These molecules of chlorine gas now bubble off at the anode. Cl + Cl = Cl2 The complete half reaction is: 2Cl? Cl2 + 2e? At the cathode there is preferential discharge of ions, according to the position of the element is the reactivity series. When aqueous copper salts are electrolysed, the cations present are the solution of hydrogen ions, which come from the water, and the copper ions. ...read more.

Middle

I can therefore predict that if I double the time of the experiment, I will therefore be doubling the charge. This statement can be supported by both of Faraday's Laws. 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." CHANGE IN PLAN Due to lack of time we were given the results to the experiment using the input variable concentration and copper chloride used as the electrolyte. This obviously is not the same variable as initially planned, but this would not be of great inconvenience. In this instance the time was kept constant, and the concentration was varied from 0.25 molar to 2.0 molar. 0.25M, 0.5M, 1.0M, 1.5M, 2.0M Concerning the prediction for the concentration variable, I predict that the outcome will be just the same. The relationship between the concentration of copper chloride solution and the amount of copper deposited will be directly proportional. ...read more.

Conclusion

The same electrodes and equipment should have been used throughout. This is what could explain the anomaly ("freak" result) in the graph, at 2.0 molar concentrations. The results might have been more reliable if the experiment was left on for longer, something like 10 minutes, to compensate for the errors. Though the experiment was conducted away from windows, for wind and temperature not to impede on my results, I still believe the temperature could have been another source from which we draw the anomaly. Overall I found my results, compared to my prediction, very compelling. Although there were problems associated with the experiment, I believe the results produced are reliable and convincing. Relative to the best-fit line, the points are very near, apart from the anomaly, which, as mentioned, was probably caused by the problems encountered with the cathode. Extending the duration of time for which the current was discharged can further enhance this specific investigation. Increasing the range of concentration variables is also another possibility to advance this experiment. I found this investigation very interesting and increasing the range of variables that were used could further enhance it. I am looking forward to investigating more of the variables in this experiment, which may or may not affect the mass of copper deposited onto the cathode, such as changing the Quantity or Temperature variable. Moudud Hussain 1 GCSE Science ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Changing Materials - The Earth and its Atmosphere section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Changing Materials - The Earth and its Atmosphere essays

  1. What Affects The Rate of Electrolysis Of Copper Chloride Solution?

    The more current flowing the quicker the reaction and if the solution is less concentrated then there will be less chlorine gas let of and less copper formed so if we increase the concentration, the more chlorine gas given out and more copper formed.

  2. Investigate the factors that affect the mass of Copper deposited on the Copper Cathode ...

    The cleaned cathode is then fixed onto the holder using a crocodile clip, which is not in contact with the Copper (11) sulphate solution, only the cathode, and is then connected to the negative terminal of the power pack. The same is repeated for the anode except it is connected to the positive terminal of the power supply.

  1. The Electrolysis Of Copper (ii) Sulphate Solution Using Copper Electrodes

    The fact that the graphs don't show this doesn't contradict this statement or disprove his second prediction; in fact these differences can be very easily explained in terms of experimental error.

  2. What Effects the Reaction in the Electrolysis of Copper Sulphate.

    Using Faraday's equations I can predict results for all my planned experiments and later compare these to my actual results. My predicted results are as follows: Amount of Coulombs Change in weight accurate to 2d.p (the cathode should gain this amount and the anode should lose this amount)

  1. Investigation to show how the amount of electric current affects the amount of copper ...

    * the copper sulphate solution. This must be kept the same because if it was changed, the copper sulphate concentration in the solution may differ which would produce unreliable and inaccurate results as there may be more/less copper available for the cathode to discharge. * the distance between the electrodes.

  2. Factors affecting mass of copper transferred in Electrolysis of aqueous copper sulphate

    I am going to try and keep the temperature of the solution the same so that the ions don't gain kinetic energy and vibrate faster to move to the cathode quicker making the mass added higher. I will keep the current (0.5A)

  1. Electrolysis - The aim of this experiment is to prove that by passing electric ...

    of substance produced at an electrode during electrolysis is directly proportional to the number of electrons transferred at the electrode. The amount of electric charge carried by one mole of electrons ( 6.02 x1023electrons) is called the faraday and is equal to 96,500 coulombs.

  2. Is an increase in traffic pollution the

    Particular attention is currently on whether traffic pollution can cause asthma. A number of studies have been published by the Children's Health Study, southern California, looking in detail, at the relationship between traffic pollution and asthma. 'Recent results from this study for a cohort of 4700 children showed strong associations with medication usage (odds ratio, 1.50; 95% confidence interval, 1.16-1.95)

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work