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  • Level: GCSE
  • Subject: Science
  • Document length: 1086 words

Electrolysis Investigation

Extracts from this document...

Introduction

PHYSICS COURSEWORK. Prediction. Electrolysis is the method of using electricity to separate two solutions. This works by passing electricity through the anode, (the positive electrode,) through the solution and then back up the cathode, the negative electrode. In this investigation we will be using Sodium Chloride (commonly know as salt) to react. If the ions are positively charged then they will be attracted to the cathode, the negative electrode, and if they are negatively charged then they will be attracted to the positive electrode, the anode. When we use the Sodium Chloride then the sodium ions will be attracted to the negative electrode and the chlorine ions will be attracted to the positive electrode. If we increase the concentration then the reaction will happen faster because there are more electrons and so the chance of a reaction happening is increased. The current is the flow of Ions in the electrolyte cell, so more Ions means more current. Variables. { [image001.gif] Material of the electrode. { Concentration. { Voltage. { Temperature. ...read more.

Middle

{ Now once you have done this experiment and recorded the results. Now you will change the concentration of the sodium chloride solution by adding more or less distilled water to it. { NOTE You will need about 6 sets of different concentration results. Safety. { Wear goggles at all times. { Do not inhale the chlorine. { Do not turn the voltage up to over 6 volts. { Do not alter the power pack with wet hands. Results. Concentration. Experiment no. Current - Amps. 2 mol 1 0.67 20ml NaCl 2 0.68 0ml H[2]O 3 0.68 Average 0.68 1.75 mol 1 0.74 17.5ml NaCl 2 0.70 2.5ml H[2]O 3 0.68 Average 0.70 1.5 mol 1 2.05 15ml NaCl 2 1.98 5ml H[2]O 3 0.94 Average 1.70 1.25 mol 1 0.54 12.5ml NaCl 2 0.53 7.5ml H[2]O 3 0.52 Average 0.53 1 mol 1 0.47 10ml NaCl 2 0.45 10ml H[2]O 3 0.44 Average 0.45 0.75 mol 1 0.39 7.5 NaCl 2 0.37 12.5 H[2]O 3 0.36 Average 0.37 0.5 mol ...read more.

Conclusion

Therefore you would get a better average. In my results I did find an anomalous result, so this shows that the experiment went wrong somewhere and so the results are not perfect. I could have improved the experiment by using a larger quantity of the solution. I think the evidence was reliable enough to confirm a conclusion, because chlorine was found coming off of the anode, which means that electrolysis is a good method of separating a solution of Sodium Chloride and water. I think that to improve my experiment I would take more time to carry out the experiment and I would also use a more accurate measuring cylinder to collect more accurate results. I think that I carried out my experiment very well and I am confident that I used every safety procedure that I stated in my `Safety' section of my plan. How to extend my experiment. { I could have used a wider range of Sodium Chloride. { Use a bigger electrolysis cell so I can use a larger amount of solution. { Use a larger current. { Use different variables. ...read more.

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