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The Electrolysis of Copper Sulphate Solution using Copper Electrodes.

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The Electrolysis of Copper Sulphate Solution using Copper Electrodes!!! 1)Introduction: My GCSE Chemistry assignment is based on the topic ELECTROLYSIS. Electrolysis only occurs only in presence of electricity, and moves around a circuit. Electrolysis is defined as the flow of charge. 2)Aim: I want to find out the loss of mass of anode when electrolysing copper electrodes using copper sulphate solution for different speeds of the current. The aim for this investigation is to see how current affects the amount of copper deposited. 3)Prediction and Background Science: It is possible to predict that the relationship will directly proportional between the time the current flows and the mass of copper deposited on the cathode. Therefore I can predict that if I double the amount of current the amount of copper deposited would become higher. Both Faraday's laws therefore support my prediction: - FARADAY'S FIRST LAW OF ELECTROLYSIS STATES: "The mass of an element deposited during electrolysis is directly proportional to the number of coulombs of electricity passed." FARADAY'S SECOND LAW OF ELECTROLYSIS STATES: "The mass of an element deposited by one faraday of electricity is equal to the atomic mass in grams of element divided by the number of electrons, required is discharge one iron of the element." THE SCIENTIFIC EQUATIONS ARE: 1. ...read more.


This is why I'll be taking this into consideration. I will be using electricity to flow to flow through the circuit, which could power shock someone if hands are watery. I should also make sure that copper sulphate solution doesn't enter our bodies in any way. 8)Results Table: A table to show the amount of copper deposited in the cathode. Current (A) Amount of mass added (g) (First Test) Amount of mass added (g) (Second Test) Average Start 34.77 35.19 0.2 34.81 0.04 35.24 0.05 0.03 0.4 34.89 0.08 35.34 0.10 0.09 0.6 35.01 0.12 34.49 0.15 0.14 0.8 35.19 0.18 35.76 0.27 0.23 9)Graph: a graph to show the change in mass (g) in the cathode. 10)Method: This investigation was carried out by pouring copper sulphate solution into the beaker. The cathode electrode was thoroughly cleaned using sand paper, to clean any of the layers from pervious experiments. The cathode was then weighed , the mass was recorded in a table and placed in the beaker containing copper sulphate solution. The electrodes were connected to the ammeter, auto rip and power supply . a steady time was taken of ten minutes on the stopwatch and the experiment contained different amps ( 0.2, 0.4, 0.6, 0.8 in amps) by moving the power supply changed the moving the variable resistor I changed the power of the current in amps. ...read more.


One of these factors could have been the electrodes, which, even after a good clean were still quite dirty and obviously still had irremovable substances from previous experiments still attached to them. If this experiment were to be repeated for a second time, in need of greater accuracy, it would be imperative to have a new pair of electrodes, which have never been used before. Another factor which may have affected the overall outcome of the investigation, may have been the fact that the practical work of the investigation was carried over from lesson to lesson, meaning that variables such as the concentration or the amount of the Copper Sulphate solution could have changed between lessons. To overcome this problem, a stock solution of Copper Sulphate should have been made so as the concentration remained the same at all times. The same electrodes and equipment should have been used throughout. Also, when weighing, the same electrical balance should have been used, as there may have been slight differences between the two balances. I found this investigation very interesting and I am looking forward to investigating more of the variables in this experiment, which may or may not affect the mass of copper deposited onto the cathode, such as changing the Current or Temperature variable. ?? ?? ?? ?? Bhaktipriya Nayan Kapadia: - 10291462 Chemistry Coursework 2:- Electrolysis Page 7 of 7 ...read more.

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