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GCSE Chemistry Coursework

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Introduction

GCSE Chemistry Coursework Electrochemical Cells Investigation AIM: To find out how the voltage produced by a cell depends on its constituents. I have noticed this coursework and my previous experiment are very similar are as their aims and methods are alike. Below is my preliminary coursework. Preliminary Coursework: Teacher Demo Aim: To find out how the voltage produced by a cell depends on the electrolyte. Equipment: * 200cm3 of Sulphuric acid * 200cm3 of Potassium Nitrate * 200cm3 of Copper Sulphate * Beaker * 1 copper strip * 1 zinc strip * Voltmeter * Holder with 2 crocodile clips Method: 1. I will set up as shown in the diagram below with 200cm3 of sulphuric acid as the electrolyte 2. I will use a holder with crocodile clips to hold both metals 3. I will place the electrodes which are copper- zinc into the acid and note the voltmeter reading immediately. 4. I will then remove both electrodes quickly and wash and dry them. 5. I will repeat steps 1-4 but for Potassium Nitrate, Copper Sulphate 6. I will then repeat steps 3-7 to get second set of results Diagram: VARIABLE TABLE: Independent Dependent Control * Type of electrolyte * Voltage * Volume of electrolyte * Type of metal- copper has to be ...read more.

Middle

The time in which the metal is in contact with the sulphuric acid as a displacement reaction can happen between the metal and salt solution. This is why I have to take the metals out immediately. The room temperature must always be the same because it can speed up or slow down the reaction time in the electron flow. The same person must do the same job as different people have different methods of measuring. I must keep copper the same as this is the control metal because if I changed it my investigation would be completely wrong. SAFETY: To ensure that there is the optimum level of safety for me and others I must: Wear safety goggles to ensure that no sulphuric acid comes in contact with anyone's skin Make sure the sulphuric acid does not come in contact with anybody's skin as it corrosive. If this happen, immediately wash it off with water. PREDICTION: I predict copper-magnesium will produce the most voltage as magnesium is the most reactive metal out of the 7 metals. This is because magnesium can lose its electrons more easily than the other metals as it is the only one in group 2. ...read more.

Conclusion

Although I removed most of the oxide layer, I could not take it off. The oxide would have slowed down the flow of electrons and this why it came below zinc. Iron was another anomalous result as it should have been underneath aluminium instead of tin. This result occurred because the crocodile clip on the holder did not hold the iron nail properly since it has an awkward shape. To ensure that no anomalous results take place will make sure the crocodile clips will hold the metals correctly. I will use the same method and make sure that the oxide layer on the aluminium will be taken off. This would be my new method: 1. I will set up as shown in the diagram above with 200cm3 of sulphuric acid as the electrolyte 2. I will use a holder with crocodile clips to hold both metals 3. I will make sure the crocodile clips 4. I will place the electrodes which are copper- copper into the acid and note the voltmeter reading immediately. 5. I will then remove both electrodes quickly and wash and dry them. 6. I will repeat steps 3-6 but for tin, lead, iron, aluminium, zinc and magnesium. 7. I will then repeat steps 3-7 to get second set of results This will enable me get the results that I wanted ...read more.

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