Electrolysis of Copper in Copper Sulphate Solution
Introduction
Aim
This is an investigation into how temperature affects the amount of
copper lost from the Anode and gained on the Cathode during
electrolysis.
Electrolysis is…
The chemical change by passing electric charge through certain
conducting liquids (electrolytes). The current is conducted by
migration of ions - negative ones from the Anode (positive electrode),
and positive ones to the Cathode (negative electrode). Reactions take
place at the electrodes by transfer of electrons in the direction of
the current.
In this case, copper electrodes in a copper sulphate solution are
used.
In the electrolysis of copper, copper atoms in the Anode become copper
ions by losing electrons which go into the circuit.
Cu - 2e à Cu
The positive ions are attracted to the negative Cathode but only
copper ions are discharged.
Cu - 2e à Cu
So this electrode gets coated with copper.
Diagram
[IMAGE]
Also attached to this circuit will be a variable resistor. An ammeter,
placed in the circuit, will register the flow of current: from this
indication, the electric circuit can be deduced to be complete.Also, a
stopwatch will be used.
The 'cell' is a power pack.
Variables
The variables in this experiment are:
· The electrodes
· Resistance
· The electrolyte
· Temperature
· Position of the electrodes (Distance between)
· Time
Only the size of the electrodes and times are being investigated,
therefore in order for this to be a fair test, the other factors must
be kept constant.
The same CuSO will be used throughout, so the concentration is the
same, and the same spacing between electrodes will be used. The size
of the electrodes should be the same, but they will be reused, so the
size will change from one experiment to another.
Time intervals of 5 minutes for each experiment will be used, until it
The important parameters of a cyclic voltammogram are the magnitudes of anodic peak current (ipa), the cathodic peak current (ipc), the anodic peak potential (Epa) and cathodic peak potential (Epc). The basic shape of the current verses potential response for a cyclic voltammetry experiment as shown (Fig. 1.2). At the start of the experiment, the bulk solution contains only the oxidized form of the redox couple so that at potenials lower than the redox potential, i.e. the initial potential, there is no net conversion of oxidized species (O) into reduced species (R) (point A). As redox potential is approached, there is net cathodic current which increases exponentially with potential. As O is converted to R, concentration gradients are set up for both O and R, and diffusion occurs down these concentration gradients. At the cathodic peak (point B), the redox potential is sufficiently negative that any O that reaches the electrode surface is instantaneously reduced to R. Therefore,
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.
The experiment we did was Copper Cycle. We reverted the copper to its elemental form after a chain of reactions. We performed a series of reactions, starting with copper metal and nitric acid to form copper (ii) nitrate. Then we reacted copper with sodium hydroxide, sulfuric acid, nitric acid and zinc to form precipitates. In conclusion our percent recovery was 40.38%.
An atom, by definition, is the smallest part of any substance. The atom has three main components that make it up: protons, neutrons, and electrons. The protons and neutrons are within the nucleus in the center of the atom. The electrons revolve around the nucleus in many orbitals. These orbitals consist of many different shapes, including circular, spiral, and many others. Protons are positively charged and electrons are negatively charged. Protons and electrons both have charge of equal magnitude (i.e. 1.602x10-19 coulombs). Neutrons have a neutral charge, and they, along with protons, are the majority of mass in an atom. Electron mass, though, is negligible. When an atom has a neutral charge, it is stable.
The purpose of this lab is to determine the empirical formula of copper oxide (CuxOy) through a single-displacement reaction that extracts the copper (Cu) from the original compound. In order to do this, hydrochloric acid (HCl) was mixed in with solid CuxOy; the mixture was stirred until the CuxOy was totally dissolved in the solvent. Zinc (Zn) was then added to the solution as a way to enact a single displacement reaction in which Cu begin to form on the Zn; the Cu gets knocked off the Zn through gentle stirring. To isolate the Cu, the supernatant liquid was decanted and the Cu was then washed with first water then second, isopropyl alcohol. Once done, the hydrated Cu is transferred onto an evaporating dish where it was heated multiple times
If heat is applied to Copper (Ⅱ) sulfate pentahydrate, then the experimental form will be equivalent to the theoretical formula. Important key data that will be needed to achieve the goal of the lab experiments includes the initial mass of hydrated crystal, the final mass of anhydrous crystal, the
Volume's Effect on a Copper Sulphate Solution We are trying to find out if the current though a copper sulphate solutions volume is increased. To find this information out I shall perform an experiment using the following equipment; · 1 power pack · 1 beaker · 2 carbon rods for anode and cathode · 1 ammeter · 1 measuring cylinder · 2 crocodile clip wirers I shall also be using 60cm3 volume of copper sulphate in my preliminary results to decide upon the concentration of copper sulphate and the voltage I shall use. The following diagrams show the step by step process in which I will do my experiment; [IMAGE] [IMAGE] [IMAGE] [IMAGE] I will take 10 readings from 10cm3 to 100cm3. I will repeat my experiment to give my experiment a fair average. I will keep the power pack the beaker the carbon rods the crocodile clips the ammeter the concentration of copper sulphate and the measuring cylinder the same each time I do the experiment this experiment.
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.
In this lab experiment, 0.46 grams of copper went through numerous chemical reactions, including being added to nitric acid for an oxidation-reduction reaction to occur, along with going through a precipitation reaction with sodium hydroxide, a decomposition reaction, and double displacement reaction. Theoretically, if 0.46 grams of copper was at the beginning of the reaction, after going through all of the chemical reactions, 0.46 grams should remain. However, due to some loss of copper through the chemical reactions, such as through decanting, only 0.32 grams of copper remained at the end, leaving a percent recovery of around 69.56%.
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.
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.
The electrostatic precipitator (ESP) is a machine used in factories, to clean out the waste solid particle, for example ash from the exhaust gas, allowing clean exhaust gas exit through the chimney. The electrostatic precipitator functions by using first allow the exhaust gas with the waste solid particles pass through the Nozzle as shown in the diagram below. Then the exhaust gas passes through inlet gas distribution, which evenly distributes the gas as shown below in a turquoise color, and starts going through the Discharge electrodes and the collector plates, which is shown in the diagram red and blue respectively. The discharge electrodes, which are powered by high voltage direct current, ionize the gas along with the other solid waste particles negatively. The collector plates are also charged with high voltage electricity, but it is positively charged, therefore attracting the negatively charged solid particle, because oppositely charged particles attract. This allows the clean exhaust gas pass through the other end, while the solid waste particles are trapped in the collector plates. Eventually when there are enough solid waste particles collected on the collector plates, the collect plates shakes off the collected waste, where it drops to the bottom of the shaft as shown in the diagram as “Hopper”.
of Copper Sulphate. To do this I plan to work out the amount of water
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.