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To investigate the current, which flows during electrolysis.

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Introduction

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.

Middle

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.

Conclusion

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.

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