Saturday, April 13, 2013

Chemistry electrolysis coursework

It is known that by passing a constant electrical current through an aqueous copper sulphate answer that the passage of ions through this solution results in copper atoms organism dissolved into the solution from the anode while positive copper ions (cations) being discharged at the cathode. Normally anions are discharged at the anode.

The experiment carried out aimed to monitor the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when authoritative variables were changed. It was considered that the following factors could affect the deposition of Copper metal on the cathode.

1. Time

2. Current

3. Temperature

4. Molarity/Concentration of Solution

5. Quantity of Solution

6. Size of Electrodes

7. Distance amid the electrodes

8. The surface of the electrodes

The time was chosen because it is an easy quantity to poster and record, whilst at the same time maintaining the other variables at a constant level. The other factors could be observed in later(prenominal) experiments, should time allow.

PREDICTIONS

It is possible to hazard that the relationship will be directly proportional between the time the current flows and the good deal of Copper deposited on the Cathode (negative electrode). I can then predict that if I double the time of the experiment, I will therefore be doubling the charge.

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This statement can be support by both of Faradays Laws.

Faradays First Law of electrolysis states that:

The mass of both element deposited during electrolysis is directly proportional to the number of coulombs of electricity passed

Faradays foster Law of electrolysis states that:

The mass of an element deposited by one Faraday of electricity is equal to the atomic mass in grams of the element divided up by the number of electrons required to discharge one ion of the element.

Another voice of...

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