• 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: How Does Current Affect The

Extracts from this document...

Introduction

Aim: The aim of this investigation is to find out how current affects the amount of copper formed at the cathode, when using copper sulphate solution and graphite electrodes. Pre-test Results: For my pre-test, I have gathered the following results: Current Volume of Copper Sulphate Time Mass of cathode before Mass of cathode after 20.2 mA 50ml3 3 minutes 3.25g 3.27g 0.1A 50ml3 3 minutes 3.11g 3.12g 0.2A 40ml3 4 minutes 3.12g 3.14g 0.4A 25ml3 5 minutes 3.14g 3.17g 0.6A 50ml3 5 minutes 3.17g 3.19g 1A 30ml3 4 minutes 3.21g 3.24g From the pre- test, I have decided: * Time: 5 minutes * Volume of Copper Sulphate Solution: 50 ml3 * Beaker size: 100ml3 * Range of Currents: 0.1A, 0.2A, 0.3A, 0.4A, 0.6A. * Current: Amps I decided to time the reaction for 5 minutes, because with lower currents, not much copper was being deposited, so I decided t time for 5 minutes so that all the different masses could have some copper collected. Using 50 ml3 of copper sulphate solution, more ions would be present in the solution so more ions would go to the electrodes and more copper would be formed. In a 100ml3 beaker, more of the electrodes are covered in the solution, so more copper will form quicker. I decided to use these currents, because there are doubles and triples, so I will be able to find out if the mass and current is directly proportionate to each other or not. ...read more.

Middle

So the mass of 0.000621761 mol of copper is: Mol of Copper * Molecular Weight = Mass of Copper 0.000621761 mol * 64g/ mol = 0.039792746g This tells us that 0.039792746g of copper will be formed at the cathode. 0.6A= Time * Current= Charge 300s * 0.6C/s = 180.0 C Charge/Constant = Mol of Electrons 180.0 C/ 96 500 C/ mol= 0.001865284 mol At the Cathode: Cu2+ (aq) + 2e- Cu (s) 2 mol of electrons are needed to liberate 1 mol of Copper, so 0.001865284 mol of electrons will be needed to liberate 0.000932642 mol of Copper. So the mass of 0.000932642 mol of copper is: Mol of Copper * Molecular Weight = Mass of Copper 0.000932642 mol * 64g/ mol = 0.059689119g This tells us that 0.059689119g of copper will be formed at the cathode. From these figures, I can predict the shape of the graph. I predict it will go up in a positive correlation and will be directly proportionate- as the current increases, the mass does. So if the current is doubled, tripled, etc, so will the mass of copper collected. The graph below will show a similar graph as to the final graph: Apparatus: * 100ml glass beaker * 6 wires * 2 crocodile clips * 1 light bulb * 1 stopwatch- hh mm ss.ss * 2 graphite rods (electrodes) * 50ml copper sulphate solution (electrolyte) * 2 elastic bands * 1 small piece cardboard to hold the electrodes * 1 2d.p. ...read more.

Conclusion

Also because the experiment was not carried out all on the same day and equipment may have been different, therefore making a difference. The results were reliable, even though I did have a few errors which were corrected. The results did however show a clear pattern that as the current increased, so did the mass of copper collected. I could improve my method by carrying out the experiment under the same conditions every time I did it, using the same equipment, measuring more accurately and taking a bit more time, so that things would not be rushed. I could also have the room temperature constant, so that if temperature affects the reaction, then it wouldn't have much of a difference. If I were to extend the investigation to make it better, I would keep the Table of results Current- amps Volume of copper sulphate solution- cm3 Time- minutes Mass of cathode before- g Mass of cathode after- g Difference in mass- g Mass of cathode before- g Mass of cathode after- g Difference in mass - g Mass of cathode before- g Mass of cathode after- g Difference in mass- g Average mass- g 0.1 50 5 3.24 3.26 0.02 3.26 3.27 0.01 3.13 3.15 0.02 0.02 0.2 50 5 3.15 3.18 0.03 3.19 3.21 0.03 3.21 3.25 0.04 0.03 0.3 50 5 3.25 3.28 0.03 3.28 3.32 0.04 3.32 3.36 0.04 0.04 0.4 50 5 2.88 2.94 0.06 2.94 3.00 0.06 3.00 3.05 0.05 0.06 0.6 50 5 3.00 3.08 0.06 3.02 3.10 0.08 3.10 3.18 0.08 0.08 ?? ?? ?? ?? Zoya Khan 10L 1354 13228 ...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. Peer reviewed

    To find out how current affects the rate of electrolysis

    3 star(s)

    The time allowed for the electrolysis to run would have an effect on the mass of copper deposited, since the deposition of copper is a continuous process, and providing there is a fixed current it happens at a fixed rate.

  2. How does concentration affect the rate of electrolysis of Copper Sulphate solution?

    should be taken and in what order to provide the appropriate and expected results for the current generated in relation to the concentration of the solution: - First, the two 7.5cm graphite electrodes (the anode and cathode) are connected up to the current transfer box, through the ammeter.

  1. The Electrolysis Of Copper Sulphate Solution Using Copper Electrodes

    However, the resistance across the electrodes is constant (equals the total resistance of the solution, the electrodes and the crocdile clips), by the same equation, when the current is changed, the voltage must change. Current must be the same everywhere in a series circuit.

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

    The first reading: 0.2 amps Amount of electric charge = Current(A) x Time(S) 0.2 x 1200 = 240 C Number of moles of electrons transferred = 240 = 0.002487046632 96,500 At the cathode: Cu + 2e ==> Cu 1 mole of Cu ions requires 2 moles of electrons to form

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

    Instead the anode will be active and discharge into the solution the same amount of copper that the cathode gains leaving the solution at a constant morality. In electrolysis the ions allow electrons to flow around the circuit. An ion is an atom or molecule which has acquired an electrical charge.

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

    1.20 1.20 1.20 0.03 4 120 1.20 1.22 1.23 1.22 0.05 6 180 1.22 1.24 1.25 1.24 0.07 8 240 1.25 1.26 1.27 1.26 0.09 10 300 1.28 1.28 1.28 1.28 0.11 time (minutes) charge (coulombs) mass of copper at the anode (g)

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

    Each time, I will leave my experiment going for 2mins. Safety is a very important issue in every experiment. Taking this into consideration, I have taken all possible precautions to ensure the safety of myself and of others around me.

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

    The calculation involves current and time used. During all electrolysis the number of electrons lost at the anode must equal the number of electrons gained at the cathode. When the current is increased more electrons flow, that is more electrons are being passed so more ions are discharged.

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