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

To test how the amount of electricity effects the liberation of copper ions, during electrolysis.

Extracts from this document...


Chemistry course-work Electrochemistry Aim: To test how the amount of electricity effects the liberation of copper ions, during electrolysis. Scientific Ideas The prediction of this experiment should be easily done. After gathering all the information about electrochemistry and researching about redox reactions the predictions should be as accurate as possible. Two laws which need to be taken into account are that discovered by Michael Faraday. The first laws states that the quantity of material transformed at each electrode is proportional to the amount of electricity passed through. The second law states that the weight of the elements transformed is proportional to the equivalent weights of the elements, that is, to the atomic weights of the elements divided by their valences (the effective charge) i.e. the equivalent weight = ATOMIC WEIGHT CHARGE My prediction will be base on these two laws. Other background ideas which will help my attempt at a prediction is my knowledge on electrolysis and my being able to implement half - equations. Electrolysis is the passing of an electric current (flow of e-) through a liquid or molten compound dissociates (splits) in ion (charged atoms). An atom which loses an electron becomes positive (CATION) and an atom which gains an electron becomes negative (ANION) - Reduction and Oxidation occur together as opposites -: As metal copper will lose electrons at the at the same time as gaining electrons at the Cathode. E.g. Cu ? Cu2 ? + 2e- (at the Anode) Cu 2 + 2e- ? ...read more.


To enable my experiment to be a safe as possible, I will always be wearing safety goggles and keep my tie tucked inside my shirt all the time whilst the experiment is going on. I will not disturb or be distracted at any time during the experiment and handle all equipment with the utmost respect. Obtaining and Collecting Data I believe I have gained sufficient results for me to put into a table. As I have mentioned before the most significant readings are: The Number of Grams Lost at the Anode, and The Amount of Coulombs Transmitted Between Each Reading. I will plot the results of 'Grams against Coulombs' on a graph. Seconds Current Coulombs Cu at Anode(g) Total lost at (g) 0 0.5 0 0.56 0.00 300 0.5 150 0.50 0.06 600 0.5 300 0.46 0.10 900 0.5 450 0.43 0.13 1200 0.5 600 0.39 0.17 1500 0.5 750 0.35 0.21 1800 0.5 900 0.32 0.24 2100 0.5 1050 0.28 0.28 2400 0.5 1200 0.25 0.31 I am extremely confident that all of the results are accurate, this is because the same procedure took place for each reading. However, if there is to be a fault in the results this would not be a huge problem because the proportion of the results will be exactly the same which is what is required. The proportion will be the same due to the fact that the experiment was constructed in the same environment for each and every reading. ...read more.


Of course all the apparatus would be made specifically for its job, if it were to produce results of incredible high standards. I would use as little as I could of human assistance because everybody is capable of making a mistake and it is therefore more prone to error than a computer. Almost everything would be computerised in my new improved experiment. I conclude that the amount of electricity DOES effect the liberation of copper ions during the electrolysis. The amount of coulombs transferred is proportional to the amount of copper lost at the Anode. The more coulombs transferred therefore means the more copper is lost from the . If I had to improve the experiment in any way, shape, or form I would attempt to use other variables for example use Current as a variable factor instead of Time. I believe the results would be different, and just as interesting as these have proven to be. Maybe if the experiment was in a better environment, where loss of energy is at its minimum the accuracy could have improved slightly. The accuracy in this experiment was, in my opinion, as good as it could have been. This must be due to the fact that the usage of scientific ideas and planning procedure helped to get the experiment off on the right foot. The priceless information from Michael Faraday and his laws also gave me a head start. I would like to point out that the safety aspect of this experiment was respected at all times. Safety goggles were always on, and ties were always tucked in. There was never a stage in the experiment where I did not have everything under control. Dhivesh Patel 11TC ...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. An experiment to show how electroplating using copper electrodes.

    Also an increase in current means that there is more resistance which occurs in the solution. This gives out heat, which is an exothermic reaction. This meaning that there will be more collisions and more ions with enough activation energy to carry out a successful collision.

  2. The Electrolysis Of Copper Sulphate Solution Using Copper Electrodes

    Therefore, the voltage across the electrodes cannot be seen as an experimental parameter. It is, in fact, the result of one's fiddling with knob on the variable resistor. This can be tested easily by replacing the cell with a light bulb, where the resistance is constant and intensity varies with

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

    Using the current 0.4A, an average mass of 0.17g of copper was deposited on the cathode which supports my prediction that the mass of copper would increase with the current and also that the mass of copper deposited on the copper cathode using the current 0.4A is double that deposited

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

    at the cathode this must mean that the number of atoms of Copper lost at the anode must be equal to that gained at the cathode. Therefore the mass of Copper lost at the anode should equal that gained at the cathode.

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

    I can do this because I will know how many coulombs I want to pass through the circuit. Below is an example of how this can be accomplished: charge = current X time Therefore: time = charge / current

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

    will be 5 times the original (0.2A). I will repeat the experiment four times in order to enable me to calculate an average and to make sure that my results are accurate and correct. This means that I will be making a total of 20 readings which will help me draw up valid conclusions.

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

    Connect them both to the circuit and turn on the circuit using the variable resistor to allow a 0.5A current to flow. Then place the electrodes in the solution and leave the current on for 2 minutes using a stopwatch.

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

    The impure copper is the anode of the sell. The cathode is a thin sheet of pure copper. The electrolyte is copper sulphate solutions. The impure copper anode dissolved away, copper deposits on the cathode. The famous scientist Michael Faraday was research electrolysis forming Faraday's Law in 1843: This is a physical law stating that the number of moles

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