Investigating Electrolysis
INTRODUCTION: In this experiment I will be investigating how the
amount of copper affects the mass of the cathode. I will do this
experiment twice so that I have an average of my results so that they
are accurate. I have already done my preliminary work and from it, I
have noticed that I will have to make some changes with the method of
my experiment.
AIM: In this experiment, I intend to find out how much copper in the
solution affects the mass of the cathode. I will be observing to see
what is happening and exactly how much copper is being deposited on
the cathode. Out of the four variables that are listed below, I will
be concentrating on the time the electrodes are left in the solution
and the size of current that will be applied in this experiment.
VARIABLES: There are four variables, which affect this investigation.
The first variable is the size of the current applied in the solution.
As the current raises so does amount of electrons 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 the experiment is the amount of time
the experiment is carried out for. The greater the time the electrodes
are left in the solution, the more time there is for the copper to be
gathered at the anode.
The third variable that affects the experiment is the temperature of
the copper II sulphate solution. As the temperature of the solution
increases, more of the ions gain kinetic energy and begin to move
faster. This enables the positive and negative charged ions to collide
faster with the electrodes. As more of the positive and negative ions
collide, there is a greater chance for the pure copper to be formed at
the cathode.
The fourth variable the affects the experiment is the size of the
However, only experiments IV “Effect of Copper Metal” and V “Effect of Temperature” had reasonable results, so copper metal and temperature are the more effective factors. The less effective factors are the changes in concentrations of "H" ^"+" ions and "C" _"2" "O" _"4" "H" _"2" particles. This observation is represented in experiments II “Effect of "H" ^"+ " Ions” and III “Effect of "C" _"2" "O" _"4" "H" _"2" Concentration.” Both runs 2B and 2C had the fastest times of 25 seconds and 86 seconds
3. The beaker was filled with water and the metal was placed in the water.
One of the key results of the experiment was that the percent yield was greater than 107%. Often times, the actual yield is less than the theoretical yield because there may be competing reactions, external conditions may not be ideally maintained, or the reactants are not pure. However, in this experiment, the actual yield was higher than the theoretical yield possibly due to the source of errors that dust accumulated on the precipitate or some of the precipitate reacted with other elements in the atmosphere. Another key result of the experiment was that the data indicated that the reaction involved 〖Fe〗^(2+)ions because the calculated Cu/Fe molar ratio was approximately 1.07, or rounded to 1:1. This mole ratio is closer and similar to the first equation Fe(s)+〖CuSO〗_4 (aq)→〖FeSO〗_4 (aq)+Cu(s), because the Cu/Fe molar ratio is also 1:1. Therefore, the reaction with 〖Fe〗^(3+)ions did not take place since its equation – equation 2 – has a Cu/Fe molar ratio of
Although the majority of the copper remained within the beaker, some of the copper went along with the supernatant liquid that was removed. Since some copper molecules were inadvertently removed from the beaker, the overall weight of the copper later measured less than what it should have been. Another laboratory error was how zinc was not fully extracted from the solution. While taking out the zinc that was used to separate the copper ion from the chlorine ion, some residue could have been left behind. As a direct result of stirring around the solid zinc to knock off the copper, some zinc from the original piece broke off. Not knowing how much zinc was left behind likely caused the weight of the later measured copper to be greater than what it should have been. Overall, the weight variation of the copper sample, after the procedure, was not 100% accurate since it gain weight from zinc and loss some weight due to
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.
with the Cu ²+ ions, it is the dilute copper sulphate that is in an
The original solution containing potassium thiocyanate is clear and colorless. However, when iron (III) nitrate or potassium thiocyanate is added to the solution, the overall color becomes darker and more concentrated to orange then to blood red. After a short time, the solution achieves equilibrium, but not at equal concentrations. By adding iron (III) nitrate or potassium thiocyanate, the amount of reagent increases, therefore the forward reaction increases in order to generate more product and increase the concentration of product. In the equilibrium constant equation, when increasing the amount of SCN-, the denominator increases, therefore Q < Keq. In order to reestablish equilibrium, concentration of products need to increase and the concentration of reactants have to decrease through the consummation of reactants and production of
Obtain a sample of metal that has been immersed in boiling water and place it in the cup of water.
The Effect of the Amount of Sodium Chloride on the Electric Current During Electrolysis Background When an electric current passes through sodium chloride solution, chemical reactions take place at both cathode and anode. If one passes through sodium chloride solution, there will be passage of ions moving through this solution. This results in positively charged sodium ions, which have been dissolved into the solution, moving towards the cathode and deposited there. At the same time, negatively charged chloride ions will be moving towards the anode and discharged at the anode. This is called electrolysis.
“I Sing the Body Electric” is one of twelve poems that comprised the 1855 first edition of Walt Whitman’s self-published masterpiece, Leaves of Grass. Like other poems, especially “Song of Myself,” it is a celebration of life. It is hard to believe this classic was written during the Civil War era. A time historically riddled with slavery and injustice, of mass death and discord, as well as the expansion of industrialization, the movement out west and population growth. This 19th century classic defines an age-old problem. In brief, the human body is too often disrespected, abused, underappreciated, or taken for granted. According to Whitman, "If anything is sacred the human body is sacred," (Routledge, section 8), and “if the body were not the soul, what is the soul?” (Routledge, section 1). An analysis of “I Sing the Body Electric” assists us in recognizing our eternal state of existence and well-being; a state only conceived through a unified consciousness of the human body and soul. In it Whitman poetically expresses his appreciation and respect for the intricate, spiritual unification between the human body and the soul.
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
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.