• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

To investigate the current, which flows during electrolysis.

Extracts from this document...


19/02/2003 Chemistry Coursework Title: To investigate the current, which flows during electrolysis Introduction: Electrolysis is the method of using electricity to split up ionic compounds. This requires a liquid called the electrolyte which conducts electricity. List of variables: * Concentration * Voltage * Temperature * Surface area of the electrodes * Material of electrode (we will use carbon rods) It is also of importance to discuss how these variables could affect the experiment if they were to put into operation. If there is more molar concentration in the NaCl solution then this will mean that there are more ions of NaCl in the solution. When the current will be enabled and the electrodes are put into the solution then more electrolysis will happen. However this depends on the amount of current going into the solution. The amount of current going into the solution depends on the resistance of the wires because to work out the current (I=V/R) depends on the resistance. If the resistance is higher than less current is going in and if low resistance then most of the electricity is going into the solution. However voltage also has to be considered because the higher the voltage more the power of the current and this means that more electrolysis happens. However the voltage used will be a set a voltage i.e. ...read more.


that I took three measurements from a molar concentration three times in the 12 voltage region. I repeated the experiment for specific reasons. If you repat an experiment you get rid of previous errors and in this case perhaps the electrodes were not fully in. More the times you repeat an experiment more the accurate the result. I did the other experiment on two other voltages, they were 6 volts and 4 volts and the same was conducted on these two voltages as was done on 12 volts. I took three measurements of a molar concentration so I could get a good average. Safety was also considered. Within a group we set rules so we could keep safe. One of the main concerns was of electricity and chlorine gas. So we never handled anything with wet hands and for the chlorine gas concern we set a time for how long we should leave the electrodes in the solution. We said that the electrodes should be left in the solution for a maximum of ten seconds. Results: Tables to show the results of the current received when the electrode was put into increasing concentrations Current (amps) Concentration Voltage First time Second time Third time Average of results (AMPS) ...read more.


For e.g. instead of measuring 100 cm3 I could have poured in an extra 3 cm3. This would mean that the solution with the extra 3 cm3 would have more ions than the other solution which would lead to differed results. I know the results obtained were reliable because chlorine gas was given of the anode. Also the graphs show the general pattern of what was required. This means that electrolysis is a good method of separating a electrolyte such as NaCl. If I were to redo the experiment I would use a wider range of sodium chloride i.e. not just 0.5, 1.0, 1.5 and 2.0 molar concentration which I used but 0.1, 0.2, 0.3, 0.4, 0.5, 0.6, molar concentration but perhaps to an extent of 0.15, 0.2, 0.25 molar concentration to see what happens at these concentrations which will be used to show the general pattern even better. The other objective that I would do is use a different variable such as using different electrodes because you can get different material of electrodes. I used carbon rods. With this we could compare the electrodes and the overall results. I used a measuring cylinder but I could have used a burette to measure out accurately 100 cm3. Generally I feel the experiment was very good because two of the three graphs showed what I expected. ...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. GCSE Chemistry - Electrolysis Coursework

    It has also been discovered that the copper anode releases copper ions and electrons, which form copper at the cathode. At the anode (+): Cu(r)

  2. Investigating how the amount of copper affects the mass of the cathode

    I also used a larger size current because I had noticed that previously I did gain enough copper on the cathode when the current was around 0.3amps. Therefore, I started from 0.5 amps and increased it by 0.1 amps after each ten minutes.

  1. GCSE Chemistry - Electrolysis Coursework

    It was necessary to have a rough idea of how the results would turn out. This is possible to work out by using a series of simple of equations: � Charge (C) = Current (A) x Time (sec.) � Moles of Electrons or Faradays = Charge (C)

  2. Investigating how the voltage produced by a simple cell is related to the reactivity ...

    * Tin * Lead * Silver * Platinum Low reactivity Order of my results measured in volts High voltage * magnesium * Zinc * Aluminium * Lead * Iron * Tin * Platinum * Silver Low voltage Evaluation My experiment produced sufficient evidence for a firm conclusion as I tested 8 metals taking 24 readings.

  1. Extraction of Metals.

    At the cathode: Na+(l) + e- Na(l) Sodium is extracted from sodium chloride in a Downs cell (right). Electrolysis is used for the most reactive metals as carbon will not displace them. The most important of the reactive metals is aluminium. Aluminium has many useful properties, it conducts heat and electricity well, it has

  2. Investigation into Electrolysis

    transferred at that electrode. Potassium Nitrate is a powerful oxidizing agent, containing ions which create soluble compounds and thus the adding of this substance to a solution would not cause any precipitation but rather add further ions to the possible reactions.

  1. Making an electric cell

    No - it wouldn't work! Any probe you put in is going to have a similar sort of equilibrium happening around it. The best you could measure would be some sort of combination of the effects at the probe and the piece of metal you are testing.

  2. Investigate the effect of the amount of sodium chloride, i.e. concentration gradient, in the ...

    electrode holder to fix the electrodes so the electrodes' distance and size won't change significantly. Finally, tap water contains magnesium and other impurities, therefore I will use distilled water throughout the experiment. Apparatus and Materials 1. Electrode holder 2. scale 3. crocodile clip 4. graphite rods 5. volumetric flask 6.

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