Copper Essays

completed a series of chemical reactions to demonstrate the properties of pure copper and compounds derived from copper. A sample of 0.04 grams of copper was put in a test tube to undergo five different chemical reactions including decomposition, single-displacement and double-displacement. The first reaction consists of adding 40 drops of nitric acid to the copper sample. In second reaction, 6 moles of NaOH was added to the copper nitrate to produce Cu(NO3)2 and then centrifuged, with balanced test tubes

Copper is an element and a mineral important to our everyday lives. Because copper is stable, it can be used in jewelry, coins, wiring, and statues. It’s one of the well-known metals due to its reddish brown metallic color. Because copper has high ductility, malleability, thermal and electrical conductivity, and resistance to corrosion, it is a major industrial metal. Copper is one of the oldest metals, dating back more than 10,000 years ago. In ancient Egypt, many used everyday items created of

done with copper metal. Several reactions were ran with it, which produced different copper compounds to in the end finally recover the original amount of copper. This experiment is important because it proved the Law of Conservation of Mass. The Law of Conservation of Mass states that mass is neither created nor destroyed. So after the last reaction is done there should be the same amount of copper as there was before you began. Material: Beaker Evaporation Dish Pipette Metal Copper Nitric

1. If you began with .5296 g of copper mesh and recovered .2937 g of elemental copper, what would be the percent recovery of the copper metal? 55.45% 2. Describe the difference in the appearance of the copper mesh vs. the appearance of the elemental copper at the end of the reaction sequence. The elemental cooper was bright and gleaming while the copper mesh was more of a dark brown. They also had two vastly different textures, the texture of the copper mesh was grainy and the elemental cooper

Abstract: Pure elemental copper was cycled through a series of five chemical reactions and changes in the physical properties of the solution (or precipitate) was observed. Using a variety of methods such as precipitation reactions, acid-base reactions, and oxidation-reduction (or redox) reactions, copper was converted and transformed into different states, including solid compounds and ionic form. After all the transformations, it was concluded that the percent recovery of copper was 126%, which was

Copper Transformations Prelab Questions Three metals ions are Magnesium, Iron, and Nickel. Iron is used in the sea with iron rich minerals, for substances. Iron was also used in the formation of earth. Magnesium is used in cells of every organism. It helps balance out the functions within the cells. Nickel is used for light absorption in natural environments. Nickel is also used in rings for a cheap substance rather than silver or gold. The material needed for this experiment include a 100mL

Introduction to Copper (57) Copper is a red-brown metal which is a solid at room temperature and has high boiling and melting points. While humans have been mining copper for a long time and we have used it in many different ways, the mining of copper can be extremely dangerous if an incident were to take place. Historical and Contemporary uses of Copper (186) Historical uses Copper was one of the first metals mined by man (Geoscience, 2015), with its original uses being making early coins and and

Copper ore Copper is typically extracted from oxides and sulphite ores which could be either chalcophite ,chalcocide or covellite and this ore contain about 0.5 and 2.0 percent of copper Concentration by Flotation • Copper ore consist of some of the unwanted mineral and the first step is to remove some of those, this is done by floth flotation • Then ore crushed by a series of cone crusher and further grinded into smaller pieces using milling equipment altogether with water to reduce the dust a

Decomposition of copper sulfate pentahydrate (CuSO4●5H2O) Introduction: By now, you are aware that scientists apply heat to substances in order to decompose them. In this lab, you will apply heat to make copper sulfate pentahydrate (CuSO4●5H2O) undergo a decomposition reaction. You will make observations and will have to make an educated claim about the products of the decomposition reaction. Furthermore, you will have to use your observations as evidence and will have to discuss your reasoning about

CHEM 316 Monday 12-3:50 February 15, 2017 Analysis of Copper in a Penny by Atomic Absorption Spectroscopy and Ultraviolet-Visible Spectroscopy Introduction: The United States cent coin, also known as the penny, was originally composed of pure copper from 1793 to 1837 and the composition of copper in the penny has been diminishing since. For the next 145 years, the penny’s copper composition wavered between 95% and 88% until 1982 where the copper composition was reduced to 2.5% while the rest of penny

There are many types of global distribution that take place all over the world. These include Iron Ore deposits, Copper, Gold, Silver, Platinum, Manganese, Tungsten, Chromium, Nickel, Cobalt, Bauxite, Lead, Zinc, Tin, Mica, Asbestos, Gypsum, and Diamond. Most of these mineral deposits can be found in many places all around the world. These minerals can have huge effects on the Earth and the people who live around the areas that these minerals are found. When these minerals are mined this can

Ashley Wilson 5 March 2018 General Chemistry Lab – Section 202 Experiment 7- Copper cycle Purpose: A series of reactions that convert a piece of copper metal, via several different copper- containing compounds, back into its original elemental form will be observed. Copper wire was dissolved in nitric acid. NaOH was then added to the dissolved copper solution, precipitating into Cu(OH)2. The precipitate was then placed on a hot plate and stirred until it became CuO. After sitting , the CuO was

mineral sample (Malachite), and a rock sample (copper ore). Through the process of spectroscopy, the students were able to determine the percent of copper that each sample yielded. The students were also able to apply the information to the theoretical value of copper in malachite to determine the percent error of the mineral mass percent. Furthermore, the methods used in the experiment provide insight into how mining companies determine whether a copper ore mining site will be profitable or not. Mining

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. Roasting is one which was performed in this lab involving the heating of the ore to decompose unstable ions which are bonded to the metal. Smelting is the other process

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

Identifying reaction types and calculating percent yield after multiple chemical reactions of copper metal *Ashlyn Langner and Katherine Rumfield Chemistry 111 Section 524 Introduction A topic of interest in science is the evaluation of the law of conservation of matter through different types of chemical reactions and determining the percent yield resulting from these reactions. This law states that after a chemical reaction, matter should neither be created nor destroyed. This experiment allows

Cu(NO3)2, the mass of the copper wire was taken in an analytical balance so that it can be compared to the final mass of copper at the end of the experiment. The copper wire was bent slightly and was laid flat in a 250 mL beaker so that the 16 M HNO3 solution could cover the whole wire. In the fume hood, a disposable pipette was used to distribute about 4 mL of 16 M HNO3 into the beaker with the copper wire. The solution was stirred by rotating the beaker until the copper wire had completely dissolved

reacting the two to create copper. Because of the law of conservation of mass, the creation of copper had to take mass from one of the reactants, in this case, iron. We observed the mass of the iron nails decrease between the start and the end of the lab, and we then converted that mass in grams into moles of iron and did the same with the amount of copper that we recorded after the decanting process. We used these two measurements to calculate the mole ratio between iron and copper. By doing this, we were

is more active than Copper (Cu) due to single-replacement reaction that took place. Lead had replaced Copper in the solution. Zinc (Zn), however, had replaced Lead thus leaving Copper to be the least active leaving Zinc to be the most active out of the three. In order of activity from least active, to most active, the metals would be lined up as following: Ag, Cu, Pb, Zn, Mg. From this lineup, it was be determined that hydrogen is more active than the elements silver and copper yet less active than

The copper(II) metal complex was prepared by reacting copper(II) chloride and sodium saccharinate together by applying heat. The copper(II) chloride was originally a white solid and the sodium saccharinate was a blue solid. A centigram balance was used to weigh out a 1.01g sample of the sodium saccharinate and a 0.75g sample of the metal salt, copper(II) chloride. Each reactant was placed in separate 50-mL beakers and then dissolved using 10 to 20-mL of deionized water. Once dissolved the reactants