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
When a solution conducts electricity, the charge is carried by ions moving through a solution. Ions are atoms or small groups of atoms that have an electrical charge. Some ions have a negative charge and some have a positive charge. Pure water contains very few ions, so it does not conduct electricity very well. Not all substances are made up of ions. Some are made of uncharged particles called molecules. Sugar is such a substance. When sugar is dissolved in water, the solution does not conduct electricity, because there are no ions in the solution. That's why in Hands-on Squishy Circuits, the sugar PLAY-DOH did not produce electricity. The salt had ions in it to produce the electricity needed to make the LEDs light up.
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 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.
Metals contain a sea of electrons (which are negatively charged) and which flow throughout the metal. This is what allows electric current to flow so well in all metals. An electrode is a component of an electric circuit that connects the wiring of the circuit to a gas or electrolyte. A compound that conducts in a solution is called an electrolyte. The electrically positive electrode is called the anode and the negative electrode the cathode.
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 -..
Investigation of Positively and Negatively Charged Electrons To try and find out if positively charged electrons deposit to the negatively charged electrons. This means, the electrons in the cathode attract electrons from the anode so they move towards the cathode from the anode. Prediction: I think that as the electrons move from the anode to the cathode, the mass of the anode to the cathode, the mass of the anode decreases whilst the mass of the cathode increases. I can support the point I've made above by faradays law which is: Faraday's Second 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 by the number of electrons required to discharge one ion of the element. " Hypothesis: The mass of the anode should decrease whilst the mass of the cathode should increase because positively charged electrons get attracted to the negatively charged electrons.
Copper Oxide + Carbon Dioxide (CuCO3 = CuO + CO2) The reactivity series determines how fast this reaction occurs. The reactivity series is the order of metals in the periodic table. The most reactive metals are placed at the top of the reactivity series.
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.
== == I completed a table to show my results, here is the table: Table 1. Results of different changes of substances Part A Copper (II) Sulfate and Water Reactant description Water (reactant): Color: Colorless Transparency:
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
At the cathode the hydrogen ions gain an electron. They are discharged and are converted into hydrogen gas: 2H (+) + 2e (-) → H2 At the anode, the hydroxide, not the sulphate ions are discharged. Water and oxygen gas are formed: 4OH (-) → 2 H2O + O2 + 4e (-) The hydrogen gas can be collected and measured. The greater the volume of hydrogen gas formed over a set period of time, the faster electrolysis is occurring.
Mechanism : The metal which is higher in electrochemical series forms the anode and the metal which is lower in electrochemical series forms the cathode. The difference in electrochemical potentials of the 2 metals generates a potential difference between them. The potential difference between two dissimilar metals is the driving force for the destructive attack on the active metal (anode). Current flows through the electrolyte to the more noble metal (cathode) and the less noble (anode) metal will corrode. The conductivity of electrolyte will also affect the degree of
Time - The longer time can let more copper ions from the anode to the cathode if the current are the same. There are still more factors which can affect the mass deposited during electroplating. 3). Distance between two electrodes - If the distance between the two electrodes is greater, the copper ions require to travel more from the anode to the cathode.