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. Whereas
the 1.0 mol and 0.5 mol concentrations increases steadily at a slower
rate. This obviously shows that if the voltage increase, the weight
also increases. Hence I can conclude; the higher then voltage and
concentration, the more copper is produced. The reason for this would
be because we used electrolysis. This is used to separate metals from
their ores and metal compounds. The electrolyte (solution) contains
negative and positive ions. For electrolysis to work there must be the
same amount of positive ions to negative ions so that the solution is
electrically balanced. A solution of metal compounds can only conduct
electricity if it is balanced. The negative ions are attracted to the
anode (+ve electrode) and the positive ions (protons) are attracted to
the cathode (-ve electrode). The electrolyte effect the amount of
atoms attracted.
This happens at the cathode:
Cu2+ +2e- =Cu
And oxygen is produced at the anode.
Increasing the concentration is more affective than increasing the
voltage but in order to gain more copper, you will need the highest
The Method of Extracting Copper and Gold by Bacterial Leaching The methods of extracting gold and copper have significant differences and therefore require separate attention. Prior to leaching occurring, either a tailings pile must be built up upon a base of impermeable rock or a series of holes drilled into the ore, to provide access for the bacteriaα. [IMAGE] At process one the bacteria thiobacillus ferro-oxidans and thiobacillus thio-oxidans, naturally occurring bacteria that obtain the energy that they need to survive by oxidising Fe2+ and S2- ionsα, are added to the copper ore. The bacteria in the acidic leaching solution then convert the insoluble sulphide minerals into a solution containing Cu2+, Fe2+, Fe3+ and SO42- ions. The acidic solution provides the optimum pH for the bacteria to work at. Following the bacterial action, the solution is drained off of the impermeable rock or pumped out of the ground through the remaining holes and the remaining solution prepared for concentration and extraction of the Cu2+ ions.
The percent error or percent yield between the theoretical yield of Cu produced and experimental value of Cu produced was approximately 107 %. One source of error, which was a scientific error, was that leaving the Cu precipitate in the cupboard for week allows dust to accumulate on the sample. When dust accumulates on the Cu precipitate for a period of one week, it adds additional mass when weighed. This is because dust has mass, and as more and more dust accumulate, the accumulation of dust will have a greater mass. As a result, the experimental mass of Cu produced would be greater than the theoretical value of Cu produced in the reaction since the precipitate weighed on the electronic balance is also considering the mass of
in the experiment of the Atomic Wight of the Element Silver. We react excess amount of copper with silver nitrate solution. To determine the amount of copper reacted and silver that is produced. The first thing that we did was rinsed 150 ml beaker with distilled water. Second, we dispense 10.00 ml of silver nitrate into rinsed beaker. Then we added 100 ml of distilled water to the beaker. Third we obtain a precut copper wire and then winded around large wide mouth test tube to produce a helix or coil of wire. After that we weighed the wire which is 2.1290g in balance number 5. Fourth, we placed the copper wire in the beaker containing dilute silver nitrate solution at 11:30 and then we taped on the copper wire to dislodge the silver metal into
The expected moss of anhydrous copper (II) sulfate should have been .834g instead of .694g. The water lost through the heating should have been .471g instead of the .694g that was actually lost. The water lost was much larger while the mass of the anhydrous copper (II) sulfate was much smaller. If the mass of the water lost was too low than something that could have caused this is that the hydrated copper (II) sulfate was not heated correctly. Not all of the water would have been evaporated if the crucible was taken off the Bunsen burner to soon. If the mass of water lost was too large than something that could have caused this is the loss of copper (II) sulfate during the experiment. This could have occurred through the mixing of the hydrated copper (II) sulfate while it was burning on the Bunsen burner.
TIME - 1 minute. The longer the ions have to move, the more copper is
The Decomposition of Copper Carbonate Copper has two oxides, Cu2O, and CuO. Copper carbonate, CuCO3 decomposes on heating to form one of these oxides and an equation can be written for each possible reaction Equation 1: 2CuCO3 (s) [IMAGE] Cu2O (s) + 2CO2 (g) + 1/2O2 (g) Equation 2: CuCO3 (s) [IMAGE] CuO (s) + CO2 (g) The aim of this investigation is to prove which of these two equations is correct. From the equations above we can see that in both reactions gas is evolved and by collecting the volume of gas produced we can accurately say which reaction is taking place. To find which equation is correct, we can use ideas about the mole and the volume one mole of gas occupies at standard conditions. Background Information Basic copper carbonate occurs in nature as the mineral malachite (CuCO3) it can be synthesised in the laboratory regardless of its source; basic copper carbonate has the same composition (CuCO3).
Investigating How the Current Affects The Mass Of Copper Collected At The Cathode. Aim: To be able to The aim of this investigation is to find out how current affects the amount of copper formed at the cathode, when using copper sulphate. solution and graphite electrodes. Pre-test Results -..
are left in the solution, the more time there is for the copper to be
Copper Sun is a book about a fifteen year old girl named Amari who was stolen from her village by white slave traders, and lived a horrible life as a slave until she finally escaped.
E_cell^o was determined to be 0 V since the same metal was used as the electrodes. In doing so, the differences in the standard reduction potentials was 0 V. The R value, the ideal gas constant is given in 8.314 J/(mol K), T is the temperature at standard conditions (298.15 K), n is the number of electrons transferred (2 in this case), and F is the Faraday Constant of 96485.3399 J/(V mol). The reaction quotient, Q, was determined to equal the concentration of the concentrated Copper ion divided by the diluted Copper ion concentration (Q=([Cu_diluted^(2+)])/([Cu_concentrated^(2+)])= .05 M). The average corrected Ecell was found to be .042 V, givng a 10.52% error when compared to the theoretical
When consider about the electroanalytical methods in analytical chemistry, there have a wide variety ways to think of. For example, there has a lot of voltammetry that can be considered in application such as cyclic voltammetry, square wave voltammetry, linear sweep voltammetry, staircase voltammetry. All these methods are widely used in several aspects of analytical ways in modern society. For example, by using the voltammetry can judge the electrode surface reaction process, the reversible or irreversible of the electrode reaction, the feature of the catalytic reaction of the cyclic voltammetry, and setting a condition for the organic synthesis. Also, the cyclic voltammetry is used the data of current and the potential to analysis. Therefore, using voltammetry methods is a common and useful ways nowadays.
of Copper Sulphate. To do this I plan to work out the amount of water
Cyclic voltammetric and amperometic measurements will be performed to measure and detect the current at the working electrode and plotted versus the applied voltage. Electrochemical window of working electrode and electrolyte solution can examine the oxidation/reduction peak of redox species. If absence of redox analyte the cyclic voltammogram will form rectangular shape as voltage constantly varies the current will get to steady state. GO (0.5 g/mL) will be added in to 0.05M Sodium Perborate (PBS) solution. 30 continuous Cyclic voltammograms will be executed in the potential range between 0 to -1.5 V while scan rate at 30 mV/s. A cathodic peak will emerge at -1.0 V with an onset potential of -0.75 V during first cathodic potential scan. Cathodic peak will be disappearing completely after several cycles.
To investigate the temperature change in a displacement reaction between Copper Sulphate Solution and Zinc Powder
Electrolysis Investigation Planning In this investigation, I will assess how changing the electric current in the electrolysis of acidified water affects the rate at which hydrogen gas is produced. The solution to be electrolysed is made up using acid and water. It is of little consequence what acid is used however in this case I will use Sulphuric acid (H2SO4). When H2SO4 is put in water it is dissociated and forms ions: H2SO4 → 2H (2+) + SO4 (2-) Ions are also present from the water in the solution: H2O → H (+) + OH (-) During the electrolysis process, the positive hydrogen ions move towards the cathode and the negative hydroxide and sulphate ions move towards the anode.