The Alternating Chemical Reactions Of The Copper Cycle Essay

***Repeat steps 2-4 for each of the following: 5 mL of oil and 2 g each of cornstarch, sodium chloride, and sodium bicarbonate.

The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu

For our science assessment we had the task to research about a metal of our choice. Since I am really into computers, I chose copper. A metal used in all kinds of wires, cpu’s and other stuff without a computer wouldn’t work. This fits really well into what we have to do for the second part, describe how this metal has helped human society.

The purpose of the experiment was to test the levels of water contamination in each beaker to see how high each vial would contaminate the water based on the color the water became once each vial was poured into the given beakers. In Experiment 2: Water Treatment, I used potting soil, sand, activated charcoal, gravel, alum, bleach, and beakers with my own-supplied tap water. The purpose of this experiment was to see if the different particles placed in the tap water could be removed by various filtration techniques. In Experiment 3: Drinking Water Quality, I used several various test strips, each individual strip testing for ammonia, chloride, 4-in-1, phosphate, and iron, along with samples of Disanti bottled water, Fiji bottled water, and my own tap water from home. The purpose of this experiment was to determine if bottled water is any more or less filtrated than my own tap water at home.

Before the synthesis of the Copper Iodine Compound, the identities provided (CuNO3)2 and Nal weighed 1.65 g and 4.7 g, respectively. After being weighed, the (CuNO3)2 exhibited a blue color, while the Nal, through observation, was a white color. However, when both identities were combined, the product turned into a brown and red rocky material. Once 20 mL of deionized water was added, the product quickly turned pale pink paste. After the solution was repeatedly washed with a total of an additional 100 mL of deionized water, the product was powdery and pink with small grains, and was left to air-dry. Once the product was air dried, it was observed to be a pale pink color, while the filter paper was stiff as the product was hard and dry. Therefore, the solid was scraped off onto a recrystallizing dish. However, the mass of an empty recrystallizing dish needed to be recorded in order to compare how much of the synthesized copper iodide was obtained. Within this case, the empty recrystallizing dish used weighed 32.01 g, the product on the empty dish weighed 1.03 g, having a total weight of 33.04 g.

Introduction: Metallic copper and its compounds have played an important role in history, from ancient civilizations to today’s economy. It also has biological and environmental significance. In this experiment, we explored copper in its metallic and ionic forms and examined the reactions which form metallic copper and copper compounds as well as calculated percentage yield of final metallic copper product. Materials and Methods:

The experiment was composed of a series of five successive reactions that utilize five complementary reagents to produce four different copper compounds before reverting it back to its original form. The first chemical reaction that was completed was an oxidation-reduction reaction between copper (Cu) and nitric acid (HNO3), where copper was the reducing agent, the substance that loses electrons for reduction to occur in another substance, and nitric acid was the oxidizing agent, the substance that gains electrons the donated electrons so that reduction can occur in another substance. During this reaction copper was oxidized from an oxidation state of 0 to an oxidation state of +2, which resulted nitric acid becoming reduced. In addition, this

There are three main parts of an atom, they are the proton, neutron, and electron. The proton and neutron are in the middle of the atom in a nucleus, that's why they're called nucleons. The electron is on the outside around the nucleus, it's a negative charge while a proton is a positive charge and a neutron has no charge. Copper has six isotopes and the atomic number is 29 with the element symbol Cu. Is in group 11 and period 4. Copper is one of the most important metals, it conducts good electricity and heat, it was one of first metals a human ever used. It's also one of the softest and bendable element there is. Isotopes are different from each other depending on the amount off mass. Since the atomic number of copper is 29, it has 29 protons

Since ALS has been founded in mid nineteen centuries, it has been known one of the diseases which has no treatment. However, recently a hope can shed light on the ALS patients. According to Beckman who are in the research team at Oregon State University, ALS will be treated soon based on their research even though their result was from one type of mouse model. He explains that the research they conducted is how to stop the progression of ALS in mice by using a compound which is called copper-ATSM. Many people might think that copper is a toxic substance, but a small amount of copper is a necessary element for human beings to live. According to their research, the treatment, copper-ATSM, can support to transfer copper directly to specific cells with impaired mitochondria and affects the spinal cord where is needed to supply the proper amount of copper to stabilize SOD. This is a significant finding because the appropriate function

Experimental Objectives: Copper belongs to group 11 and is also known to be the least reactive of the first row metals. It is the only d-block metal in the first row that has a stable 1+ oxidation state however in comparison to its +2 state, the former is seen as unstable. Cu(0) is rarely stable (2) and hence this is why it is not abundant in nature, and instead is generally extracted from ores via leaching or roasting methods. It is the +2 oxidation state that seems to dominate the majority of aqueous copper chemistry with the characteristic blue colour of most copper solutions being an indicator for the presence of the hexaaqua copper (II) ion (1).The aim of this experiment was to perform reactions to demonstrate the reactivity of copper

     Copper is one of the earliest elements known to man. Because of its distinct red color, Copper is very easily identified. In the ancient times, copper could be found lying in the ground in its unattached state without interaction to other substances. Copper and its compounds have many uses in today’s society.

It is also not sufficient to simply consider the stability of a compound with respect to its elements. It is necessary to consider the stability of copper (I) oxide with respect to copper (II) oxide, as well as with respect to copper and oxygen. It would also be important to consider the stability of CuCO3 with respect to both oxides, to see which reaction is energetically most likely. So it is clear that the value of ΔHf suggests that Cu2O will be formed, but that this will not necessarily be the case because of the other factors involved. Copper (II) compounds are by far the most common they are called “cupric”.

For all of the tests conducted, the same apparatus was used, and the sample materials in the system were not altered between any of the tests. Seeing as the same apparatus was used for all tests, the inner chamber diameter of 2 inches remained constant for all tests. Additionally, the apparatus was purged with nitrogen immediately before the start of each trial to ensure that diffusion did not begin before the start of the timer. The information that was recorded for each test included the elapsed time, the weight of the condenser both before and after collecting the vapors, and the distance from the point of collection to the gas-liquid interface. In addition, the room temperature and pressure was recorded each day due to the role of these measurements in calculating the predicted values.

To one mL of the sample, ethyl acetate, two mL of 25% sodium hydroxide (NaOH) was added. The mouth of the test tube was covered with a marble and was heated in a boiling water bath for five minutes. The mixture was neutralized with 10% HCl solution. The odor was observed with a wafting motion.

Table 1: The physical observations of the reactions of Cu(s), Mg(s) and Zn(s) with CuCl2(aq), ZnSO4(aq), MgSO4(aq), SnCl2(aq), FeSO4(aq), HCl(aq) and H2O(l).