Electrolysis Investigation
Aim
To investigate how voltage affects the amount of a copper (Cu)
deposited during electrolysis of copper sulphate solution (CuSO4).
Variables
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TEMPERATURE - Approximately 20° centigrade.The higher the temperature,
the faster the ions move through the solution. Thus, more copper is
deposited in the given time period.
ELECTROLYTE (CONCENTRATION) - 100g per litre. The denser the solution,
the slower the reaction. The slower the reaction, the less copper is
deposited in the given time period.
VOLTAGE - (Input / Key Variable) 1-5 volts. The higher the voltage,
the faster the ions move. The faster ions move, the more copper is
deposited in the given time period.
TIME - 1 minute. The longer the ions have to move, the more copper is
deposited.
ELECTRODES (AREA) - 211.2cm³. The larger the electrode, the more
copper can be deposited on it and faster.
ELECTRODES (DISTANCE APART) - 5cm. The further apart the electrodes,
the further the ions have to travel, and so it takes longer for the
copper to be deposited and the less copper can be deposited in the
given time period.
Prediction
I predict that the higher the voltage, the faster the ions in the
copper sulphate solution will move and so deposit more copper at the
cathode in the given time period. If I decrease the voltage less
copper will be deposited. Below is some scientific theory to back up
my prediction.
Scientific Theory
Electrolysis is the process of decomposing compounds by electrical
energy. An element is produced at each electrode. In my experiment the
copper sulphate will start to decompose. At the cathode copper will be
formed. Oxygen will be formed at the anode. This causes the anode to
wear away while the cathode gains mass.
According to Faraday's second law of electrolysis, "The quantity of a
substance that is electrolysed is proportional to the quantity of the
electricity used." It follows that the speed at which a substance is
The objective of this lab was to calculate the ratio of the copper sulfur compound to conclude whether the compound is made of copper I or II.
One of the key results of the experiment was that the percent yield was greater than 107%. Often times, the actual yield is less than the theoretical yield because there may be competing reactions, external conditions may not be ideally maintained, or the reactants are not pure. However, in this experiment, the actual yield was higher than the theoretical yield possibly due to the source of errors that dust accumulated on the precipitate or some of the precipitate reacted with other elements in the atmosphere. Another key result of the experiment was that the data indicated that the reaction involved 〖Fe〗^(2+)ions because the calculated Cu/Fe molar ratio was approximately 1.07, or rounded to 1:1. This mole ratio is closer and similar to the first equation Fe(s)+〖CuSO〗_4 (aq)→〖FeSO〗_4 (aq)+Cu(s), because the Cu/Fe molar ratio is also 1:1. Therefore, the reaction with 〖Fe〗^(3+)ions did not take place since its equation – equation 2 – has a Cu/Fe molar ratio of
The focus of the experiment will be a hydrate of copper (Ⅱ) sulfate (CuSO4 ᐧ5H2O) The object of this experiment will be to find the experimental formula for the hydrate of CuSO4 by heating the crystal to dryness. The success of the lab will be determined by how accurate the experimental formula is compared to the actual formula.
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are left in the solution, the more time there is for the copper to be
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The Electrolysis of Copper Sulphate Aim Analyse and evaluate the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. Results Voltage across Concentration of solution electrode 0.5M 1.0M 2.0M 2 5.0 10.6 19.5 4 10.5 19.8 40.3 6 14.3 26.0 60.2 8 15.2 40.4 80.3 10 15.0 40.2 99.6 12 15.1 40.0 117.0 Analysing/Conclusion The input variables in this experiment are; concentration of the solution and the voltage across the electrodes. The outcome is the amount of copper gained (measured in grams) at the electrodes. By analyzing the graph, we can see the rapid increase of weight gained for the 2.0 molar concentration as the gradient is steeper.
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