Chemistry Synthesis Essay

In this experiment an elemental copper was cycled a series of five reactions where it ended with pure elemental copper as well, but at different stages of the cycle the copper was in different forms. In the first reaction, elemental copper was reacted with concentrated nitric acid where copper changed the form from solid to aqueous. Second reaction then converted the aqueous Cu2+ into the solid copper II hydroxide (Cu(OH)2) through reaction with sodium hydroxide. The third reaction takes advantage of the fact that Cu(OH)2 is thermally unstable. When heated, Cu(OH)2 decomposes (breaks down into smaller substances) into copper II oxide and water. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion (Cu2+). The cycle of reactions is completed with the

The experiment was initially done by preparing standard solutions of different volumes of Cu(II) stock solution of known concentration including a blank solution composed of ammonia and water. Each volume of the solution was placed in volumetric flasks, and in each flask, same amount of concentrated NH3 was added. The same procedures were also done in the preparation of the diluted unknown Cu(II) solution. Addition of ammonia caused the formation of deeper blue copper-ammonia complex which allowed the spectrophotometer to detect the solution easily due to increase in its absorbance. The formation of the complex is shown by the following chemical reaction:

The Cu Later lab experiment is designed to allow you to practice lab skills in implementing and performing a series of reactions. Specifically, four types of chemical reactions will occur: oxidation/reduction; double replacement; single replacement; and decomposition. You will begin with a known amount of copper metal, which, after progressing through several steps, is reproduced. In this experiment you will observe and record the various changes such as heat, color changes, and production that occur. This procedure is used to observe some chemical reactions of copper and its compounds while also performing the lab appropriately as to retain the copper as much as

The more time the copper is left in the solution, the more time there will be for the cu2+ ions to be deposited.

Purpose Statement: In this experiment, we will determine the chemical formula of an unknown hydrated copper chloride compound which is composed of copper and chlorine. We will use stoichiometry, which is the relationship between quantities of materials in a chemical reaction, to determine the chemical formula for a compound. We will use the mole to mole conversion to find the formula of a hydrated compound with the general formula CuxCly.zH2O. We will convert the masses of water, copper, and chlorine to moles of water, copper, chlorine and determine the whole number ratio of these components in the empirical formulas so we can find the empirical formula of the dehydrated compound, CuxCly and the empirical for the hydrated compound CuxCly.zH2O. Results:

The Copper Cycle is a popular experiment used to determine if an element, in this instance, copper, reverts to its elemental form after a chain of reactions. This experiment is very dangerous because of the reactions between the strong acids and bases. In this experiment I performed a series of reactions starting with copper metal and nitric acid to form copper (II) nitrate. Then I reacted copper and several other solutions such as, sodium hydroxide, sulfuric acid, ammonium hydroxide, and hydrochloric acid to form precipitates. In conclusion my percent recovery

Part A of lab (preparation of copper (II) nitrate from copper metal). Weigh out ~ 0.2 g of copper foil pieces (record to the nearest .001 g) into a weigh boat. Describe its physical appearance in the lab notebook. Pour the foil pieces into the bottom of a 10 ml graduated cylinder. Place the cylinder under the bench top snorkel. Add 3 ml of 6 M nitric acid (HNO3) to the 10 ml graduated cylinder. Use a glass rod to push down any floating pieces of copper foil. A vigorous reaction will quickly ensure. The brown gas being evolved is nitrogen dioxide (NO2). The copper is oxidized in this process, forming Cu (NO3)2. Record detailed observations of the reaction, including: initial and final color of the solutions, sounds, heat evolved, gases evolved, what happened to the metal, etc.

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper (II) sulfate, sulfur dioxide gas, and water.

These compounds are created when the copper (II) oxide is continuously exposed to carbon dioxide (CO2)and sulfur trioxide (SO3) elements in the air along with hydroxide ions (OH-)in water (H2O) over decades. To put it another way, the provided chemical equations below shows what elements reacted with copper (II) oxides to create the three compounds as they were further oxidized:

The initial mass of copper was recorded, and then compared with the mass of recovered copper at the end of the experiment. The reactions that occurred during this lab include; Metathesis reactions, which are biomolecular reactions that occur in water, Redox reactions or reduction-oxidation reactions in which electrons are transferred between reactants, Single displacement reactions, which are redox reactions where a metal replaces a metal cation from its salt, Combination reactions, which occur when two or more reactants produce on product and Decomposition reaction, which occur when one reactant produces two or more products. Table of Reactions Cycle Step # Equation Reaction Type #1 Cu(s )+ HNO3(aq)Cu(NO3)2(aq)

Our group worked with copper and magnesium metals and aqueous solution of zinc sulfate. A small strip of copper was placed into a test tube containing colorless zinc sulfate solution. A small strip of copper about the same size was place into a test tube containing colorless zinc sulfate solution.

Copper, Cu, is the natural solid form of copper with an Isometric crystal system. It is found as copper red on a fresh surface, dull brown or green on a tarnished surface with metallic luster and metallic copper red streak. The natural copper is soft and malleable at 2.3-3 on moh’s mineral scale. Copper nuggets in pure state have been found in Arizona, abundant in Keweenaw Peninsula in northern Michigan, and also found in Canada, Australia, China, Namibia, Bolivia, and Russia. Copper is mined or extracted as copper sulfide in an open pit mine. Taken in large equipment to be cleaned in steam and melted dried and cooled in molds to solidify and then sent off to be used as copper products. (Understanding Minerals and Mining through Education).

The unreasonable measures of Cu (II) particles in new water assets and sea-going biological community harm the osmose-administrative component of the freshwater creatures. Joined State Environmental Protection Agency (USEPA) has set its cooper particles allowable points of confinement as 1.3 mg/L in modern effluents. Copper were released from the diverse enterprises, for example, metal cleaning and plating showers, paints and colors, mining, purifying, oil refining, flushes as metal, compost, paper board, wood mash and printed circuit board creation. Moreover, copper is phytotoxic and to be sure, has been utilized as an algaecide to control algal blossoms. An assortment of treatment innovations have been connected for the expulsion of cooper particles including compound precipitation, particle trade, adsorption, film filtration, coagulation-flocculation, buoyancy and electrochemical advances. These techniques for Cu2+ expulsion from wastewater are descripting quickly as takes after: