... (oxidation or reduction). Who Discovered Electrolysis? A British Scientist called Michael Faraday; Faraday was born on September 22, 1791, in Newington, Surrey, England. He was the son of a blacksmith and received little formal education. While apprenticed to a bookbinder in ...

... of the production are processed into alloys. Important ores of copper Copper pyrite or chalcopyrite (CuFeS2). Chalocite (Cu2S) or copper glance. Malachite green [CuCO3.Cu(OH)2]. Azurite blue [2CuCO3.Cu(OH)2]. Bornite (3Cu2S.Fe2S3) or peacock ore. Melaconite (CuO) etc. Industrial process of copper production Metals ...

... Equation". Below, I have shown them using the example of Lead Bromide. The lead bromide is separated into molten lead and Bromide. PbBr(l) Pb(l) + Br²(g) When lead Bromide is melted, the ions are free to move towards the oppositely charged electrode, ...

... and after my tests, and compared the weight so that I could determine how much copper was deposited onto the cathode in each test. COPPER SULPHATE, CuSO , is a METAL SALT. IN SOLUTION CuSO FORMS Cu++ and SO-- IONS. AT THE ANODE: ...

... me to make a decent conclusion. If we do not control the factors apart from the concentration we are testing, you can turn around and say that it was the other factors that had caused the difference and that it ...

... a variable I predict that the copper anode would decrease in mass quicker because electrolysis is much quicker when the temperature is greater. I am going to use time as my variable. I predict that as time increases there will be ...

... interfere with the experiment. They are inert electrodes. However in this experiment we are using copper electrodes. Copper electrodes are active electrodes and these metal electrodes take part in electrolysis. Copper electrodes are used in industry to obtain pure copper. ...

... it to keep the volume of water constant. * I will use an electrode holder that will hold the electrodes a set distance apart. * I will use the same power pack throughout the experiment, as not all power packs give out ...

... the electrode bridge over the beaker and adjust the two metals so that they are equally submerged under the copper sulphate. 5) Simultaneously turn on the stop clock and the power pack. Leave it for exactly one minute. To make ...

... water (which the CuSO4 was dissolved) is separated, leaving hydrogen and oxygen. Because oxygen is a non-metal it has a minus charge. In this case it has a 2-. This mean it is attracted by the positive Anode, therefore the ...

... that we knew what the experiment involved. Hypothesis: I predict that as I increase the voltage on the power pack so will the current in the current and this will pass on more electrons to the cathode, this will then increase the ...

... = 2 × 5 Q = 10 If I double the time 'Q' should double Q = 2 × 10 Q = 20 Because 'Q' is linked to the change in mass, if it is increased the mass will increase on the cathode. 'Q' ...

... other metals I am investigating (Zinc and Iron), meaning it has the ability to loose it's electrons most easily and displace the copper from the solution and make it a pure metal. The equation for this will be: Mg + CuSO4 ...

... increase. This will be because of the copper deposited on the electrode. If so this will result in the positive electrode losing weight. I predict that by the end of the experiment (40 minutes) the copper electrode will weigh between 4 ...

... something else. I predict that when the nail and nickel move further apart, the rate or electroplating will decrease, so when we weigh the nickel and iron there will be less of an increase in the weight of the iron ...

... pour into a beaker then take the temperature of the solution with a thermometer. Then weigh 2g of iron on the scales and then add it into a beaker of copper sulphate, stir it until it dissolves. After stirring it ...

... that are produced on the cathode. This means the anode loses its positively charged ions, which the cathode gains, which means more positive ions, will combine with the electrons on the cathode to produce copper. The second variable that affects ...

... identity of the metals as in my title for the experiment it suggests I do so. I will keep one metal the same (constant) and vary the other. I have chosen copper as the standard metal, as it is easily ...

... keep the size of the beaker the same as this would vary the amount of the electrode to be covered in the solution which would affect the results. · keep the size of the electrodes as similar as possible as if ...

... (the molten ore). The ore has to be melted in order for electricity pass through it. As electricity flows through the molten ore, the compound splits apart and forms ions. These ions are free to move because the ore is a ...

... down of a substance by electricity. Electrolysis only occurs in when an ionic substance is molten or is in solution, a substance that can be electrolysed is called an electrolyte. Risk Assessment I will wear safety goggles and plastic gloves ...

... down of a substance by electricity. Electrolysis only occurs in when an ionic substance is molten or is in solution, a substance that can be electrolysed is called an electrolyte. Risk Assessment I will wear safety goggles and plastic gloves ...

... electrodes These variables all have a way of changing the rate of reaction. Voltage: Changing the voltage of the circuit would affect the rate of reaction because as Ohm's law states, As charged particles try to make their way round a circuit they ...

... copper, which has a low reactivity, join with other elements only with weak bonds. Metals above copper in the reactivity series reacted to form a salt and hydrogen. For example Zn + H2SO4 ZnSO4 + H2 (From Chemistry Counts by Graham ...

... no extra mass. I will weigh them and see how much weight has been lost/gained Safety issues in this method include handling the copper sulphate (it's harmful when swallowed and may be irritating to the eyes and skin and has been ...