Introduction: In the world, there are a lot of important materials that we use in our everyday lives. Aluminum is a major metal that has many uses and is very helpful in achieving things through the use of recycling. The purpose of this experiment was to show how aluminum undergoes many chemical reactions to produce Alum. Materials and Methods: When this recycling experiment was conducted, we first had to gather the essential material needed. Once the material was acquired, 1.0094 grams of Aluminum were weighed and then transferred to a 250mL beaker. The 250mL beaker continued to remain in use for the next few steps. 1.4M KOH solution was added to the Aluminum sample that was previously obtained. For gas to escape the lab, there was a fume …show more content…
With background knowledge of chemistry, it is known that aluminum also has a molecular weight of 26.981 g/mol, which then lead to the reaction of 0.0374mol of aluminum. The first reactant was a redox reaction, formed through aluminum, adding potassium hydroxide and water to yield potassium aluminum hydroxide, plus hydrogen. During the process of this reaction, there was many changes occurring. The color of the reaction turned grey at first then eventually turned black. The solution was also evaporating due to the use of the fume solution. As the compound was reacting, the aluminum pieces were also dissolving, with only a few pieces left inside. The process of the second reaction included the adding of a new substance which consisted of sulfuric acid. The sulfuric acid along with potassium aluminum hydroxide, was yielded to produce aluminum hydroxide, potassium sulfate, and water. This reaction was both a precipitation reaction and an acid-base reaction. Once the sulfuric acid was added, the reaction became very chunky. With the use of a stirring rod, the substance went back to liquid formation. The color also turned white, as if it were milk. The solution also looked foggy, so it had to be filtered yet
After placing the aluminum in said beaker, one should gather a stir stick and stir the solution in order to speed up the reaction. One should stir the solution until there are no visible silver pieces of aluminum left in the beaker of what was the copper (II) chloride solution. When there are no visible silver pieces of aluminum left in the beaker, this means that the reaction has occurred. After the reaction has occurred, one needs to separate the products, which are copper and aluminum chloride, from each other in order to see how much copper was able to be produced. Seeing as the products are a solid in the form of copper and a liquid in the form of aluminum chloride, the process of filtration can be used to separate them.
The heating of the solution caused the reaction to start which decomposed Cu(OH)2 and made the solution colorless and darkened the precipitate. The fourth step was the formation of CuSO4. After the solution was decanted from the precipitate and washed with near boiling water, 6 M H2SO4 was added to the beaker containing Copper (II) Oxide and this caused the precipitate to dissolve and the liquid become clear blue. The last step was the formation of Cu(s). This step recovered Solid elemental copper.
Fifty tonnes of shale yielded one ton of alum, and left behind vast quarries and spoil heaps which are still visible on the hillside. The primary uses for alum were as a fixative for dyes and for softening leather during the tanning process. One of the critical ingredients used in its production was human urine! Evidently, most natural deodorants contain alum, which prevents the growth of bacteriaand eliminates the odour related to sweat; fortunately, these now utilise synthetic
To find my lab group’s ratio we took the leftover alum and placed it into a crucible and heated the crucible to figure out how much water had evaporated. We could use this later to determine the ratio. Before the crucible was heated, the mass we recorded of the crucible, cover, and alum crystals was 23.02g. Once the alum was heated everything was weighed again. We recorded that 22.34g was the new mass.
However, after refluxing for a while, yellow precipitates begin to form near the top of the flask. It was assumed that the remaining starting material was concentrated from a decrease volume to reappeared in solution. Nevertheless, this may have been a sign of contamination that will negatively affect the entire reaction. This observation later resulted in a yellowish
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
The actual yield of the reaction was 4.411 grams of copper and was obtained through the experiment
Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of
Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and
Sources: • Hydro.com – How aluminium is made This source was useful as it explains the process of how aluminium is made and what materials are used to make it. It focus’s on each part of the process explaining what material is used and how that progresses on to create aluminium. There is also an animation on the side of the website visually showing the process and the steps of making aluminium. • Zoltek.com – How is it made?
As the water was added to the heated sample, the solid copper chloride began to dissolve into a pretty blue-green solution, as a result of the compound breaking apart into individual Cu2+ and Cl- ions. When the water was first mixed with the copper chloride, it dissolved the solid pretty slowly, turning into a sort of mush at first. However, eventually, the water dissolved all of the solid copper chloride and the solution was homogenous. Since the compound just changed physical form, from solid to liquid, this change was purely physical. Just as in the first part of the experiment, the chemical character of the compound was not altered, so the compound did not experience a chemical change.
Recycling items like aluminum cans, glass, and paper keeps us from depending on the process of making these items new. Approximately Recycling an aluminum can can save enough energy to run a television for about three hours (Rinkesh 1). Recycling cans takes just five percent of the energy needed to make new cans from raw materials. Glass can be recycled over and over again. “Recycled glass takes about forty percent less energy
This indicates that the reaction has limited the amount of moles it reacts with. The number of moles in 0.3 grams of baking powder is 0,00357mole. In vinegar it is 0,8375 moles. This indicating that as 0,00357 is smaller than 0,8357, 0,00357 is the maximum amount of moles that can interact with the moles from vinegar. Therefore, once 0,00357moles have reacted of the 0.3 grams of baking powder, the reaction will stop.
Ac 2.3 Explain the method of making titanium alloy and investigate how the composition and structure of metal alloys, polymers and poly-matrix composites influence the properties of the parent material. 1. Extraction of Titanium Titanium is extracted from its ore rutile-tio2. It is first converted into titanium (5) chlorine, which is then reduced to titanium using either magnesium or sodium. The ore rutile is heated with chlorine and coke at a temperature of about 1000˚c.