ELECTROPLATING
Introduction:
Electroplating is the process of coating a metal object with another metal, using electrical current passed through a chemical solution. This process produces a thin, metallic coating on the surface of the metal object. The main purposes of electroplating are to improve the appearance of the material and provide protection against corrosion. This is done by hanging pieces of metal to be replenished in the solution. These metals are called anodes and the positive electrical lead is attached to these metals. They dissolve in the solution as metal is taken away by plating. At this point we have metal being removed from the anode and deposited on the cathode. Cathodes are the parts being plated. The anode and
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There is competition between the copper ions and the hydrogen ions. As the hydrogen ion or hydrogen redox equilibrium appears higher in the electrochemical series than the copper ion or copper equilibrium, the copper ions are preferentially reduced and copper metal is deposited at the electrode. A brown layer deposited at the cathode is observed.
After the electrolytic cell is switched off, the copper cathode are taken out and weighed. There is significant change in the mass of the cathode before and after the reaction. The mass increased by 0.16g. This increase and the brown colour shows that there is copper metal deposited at the cathode.
At the anode
In this case, the electrode is made of copper and it is easier for the copper to dissolve leaving its electrons behind on the anode than for any other ion to be released
After the electrolytic cell is switched off, the copper anode is taken out and weighed. There is significant change in the mass of the anode before and after the reaction. The mass decreased by 0.21g. This shows that there is copper metal loss at the anode as it has been oxidized to form copper(II) ions. The ions released are now motile in the copper(II) sulphate solution.
In short, copper is deposited at the cathode and is dissolved at the
To calculate the percentage of Cu, we divided the final mass of the penny 0.09 and the initial mass of 2.47 and multiplied by 100. To calculate the percentage of Zn, we divided the final mass of the penny 2.38 and the initial mass of 2.47 and multiplied by 100. During the experiment the hydrochloric acid donated its hydrogen ions in the reaction and then the chloride ions reacted with the zinc ions in the solution. Thus, the zinc dissolved in the highly acidic solution which was caused by the high concentration of H2 ions. Hydrogen gas was generated during the reaction which was seen when bubbles were formed as the penny was dissolved into the beaker.
Consequently, it induces second element to be oxidized. 2. In the experiment #3, zinc electrode acts as anode, where the oxidation processes occur, while iron half-cell acts as cathode, where the reduction processes appear. In the experiment #4, iron is visa verse reducing agent that evicts electrons to copper half-cell through the circuit.
Cadet Eric Wiggins Date: 18 September 2014 Course Name: Chem 100 Instructor: Captain Zuniga Section: M3A Identification of a Copper Mineral Intro Minerals are elements or compounds that are created in the Earth by geological processes. The method of isolating metals in a compound mineral is normally conducted through two processes.
After copper ions were filtered, approximately 15mL of .5 M was added to the filtrate, which made the mixture acidic. Then, 20 mL was added into the filtrate to raise the pH of the mixture.
After I rinsed the copper I transferred it to a watch glass that had been baked for 20 minutes so it would not contain any liquid so as to not counteract the experiment. After I put the copper on this watch glass I baked the copper in the oven for 20 minutes so there would be no liquid left in that to mess up the mass. After 20 minutes I removed the watch glass with the copper in it and weighed itm making sure to weigh the watch glass
Traveling from the U.S. mint into the hands, pockets, and wallets of citizens, ultimately, pennies will develop a dirty look due to daily interactions with their surroundings. In recent years, many have discovered possible solutions to restore the original shine of copper pennies. In order to determine what solution most effectively sterilizes our common pocket money, it is crucial to understand what makes pennies dull in the first place and what can counter this reaction. Over time, pennies receive a dark coating, creating a dull appearance.
Metal cations can be identified based on the colors they emitted off when heated in a flame.1 When atoms of the ions that were tested are excited, their electrons move up to higher levels of energy.2 When the electrons relax and return to the original states, they emit photons of specific energy creating wavelengths of light that produces colors.3 The test wire and Bunsen Burner were used to excite the solution in the crucible. The standard metal cations that were tested and their outcomes are as shown in Table 1.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
This process forms a zinc coating producing a corrosion resistant. However, A corrosion resistant is a multi-layered coating of zinc –iron alloy and zinc metal. During the galvanization process a metallurgical reaction occurs. A metallurgical reaction is a diffusion process so the coating forms perpendicular to all surfaces.
I. Purpose: To experimentally determine the mass and the mole content of a measured sample. II. Materials: The materials used in this experiment a 50-mL beaker, 12 samples, a balance and paper towels. III.
The zinc will form a new compound with the sulfate, and the copper will stay as a metal. Balanced Chemical
Stoichiometry of a Double Displacement Reaction The objective of this lab is to find the percent yield of a product of a double displacement reaction. Procedure: Refer to handout entitled “Stoichiometry of a Double Displacement Reaction” Materials: Refer to handout entitled “Stoichiometry of a Double Displacement Reaction” Data & Observations: Data Table Calculated Molar Mass of CuSO4•5H2O 249.677 g Calculated Molar Mass of CuO 79.545 g Starting mass of CuSO4•5H2O 2.050 g Mass of 100-ml beaker and filter paper 52.600 g Mass of 100-ml beaker, filter paper, and CuO precipitate 53.450 g Calculations:
The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.
Since equilibrium cannot be reached, an electrochemical driving force is generated which acts on the ions. It is derived by finding the difference between the membrane potential obtained and the equilibrium potential expected. The sign of the value of this force decides the direction of movement of ions. Since we have cations (positive ions), a positive value shows movement of ions outside the cell membrane and a negative value shows movement of ions inside the cell membrane. If the value is equal to that of the equilibrium potential, the driving force acting on the ion is 0.
The Dangers of Aluminum Wiring in Residential Homes Your electrical wiring is an important aspect of your home. And it goes without saying that having a reliable electrical wiring system that lights up and powers up your home safely should be one of your top priorities. When it comes to the materials that are used for wiring, available are plenty of options, including aluminum, copper, silver and more, with each material having its own set of advantages and disadvantages. Over the past few decades, aluminum has been a popular choice for Calgary homeowners due to its relatively affordable cost but not anymore.