Copper(II) oxide

reaction or next step. In this experiment, copper was changed through eight different reactions. Throughout the process, qualitative observations were recorded to see what effect each type of acid and decanting has on copper. All of these steps were successfully completed by using different acidic solutions and zinc to take copper through the cycle from copper solid to copper nitrate to copper hydroxide, to copper oxide, to copper II sulfate, and back to copper solid. Procedure: CHE 131 Experiment 8

2009 Lab Report #3: Copper Cycle Abstract: 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

further confirmed by the band at about 1628 cm-1. Notably, in CuO:Na5mole% and CuO:Na7mole% samples, low feature band of pristine Na2O were found. Furthermore, the stretching vibrations were clearly different from the value of Na-O in pristine sodium oxides. It might be attributed to the presence of the Na-Cu-O stretching vibrations. Conclusively, we successfully prepared CuO:Na+ nanostructures with different Na doping concentration. 3.4. Optical properties 3.4.1. Diffuse reflectance spectroscopy (DRS)

Chemistry Aim: I am trying to find out whether the equation 2CuCO3 ® Cu2O + 2CO2 + ½O2 or the equation CuCO3 ® CuO + CO2 is correct for the decomposition of copper carbonate. Introduction: This is my background research, this information may help me when I am trying to see which equation is correct. I have used the book Chemistry 1 by OCR as my reference. Relative Atomic Mass: This is the mass of an atom of the element

of basic copper carbonate 〖mCuCO〗_3⋅n〖Cu(OH)〗_2 were observed by changing the reaction mole ratio. The reaction mole ratio of sodium carbonate to copper chloride (II) was controlled from 1.08 to 1.68. Fig. 1 shows the XRD patterns of copper carbonate powder. At a reaction ratio of 1.08, paratacamite (Cu_2 Cl(OH)_3 ), beside alkali copper carbonate, was formed because of incomplete reaction at a copper content of 53.9 wt%. Lack of sodium carbonate may cause incomplete reaction with copper chloride

a low percent yield is that the starting materials did not completely react with each other meaning that the reaction did not produce the full amount of product possible, which could be avoided by allowing the reflux to continue for more time. For copper tetraphenylporphyrin the theoretical yield was 0.023g and the actual was 0.0274g, making the percent yield 118%. Possible explanation for a large percent yield could have been due to the product not being completely dry when being weighed or the presents

preservatives found in traditional makeup. It is made up of minerals such as iron oxides, talc, zinc oxide and titanium dioxide. The minerals are then ground and milled or broken into very fine particles to create the makeup (Harris, and Hicks, n.d.). Zinc oxide and titanium oxide are physical sun blockers and are used widely in mineral makeup, as well as sunscreens and other products intended to be beneficial to the skin. Zinc oxide is an inorganic compound with the formula ZnO. It occurs naturally as the

test in order to determine the identity of an unknown copper mineral. I determined that the most useful of these tests in determining the mineral was roasting because it provides a fairly accurate percent composition of copper in the unknown mineral. Results: The purpose of performing the variety of tests that we did was to give more accurate results of what the unknown mineral was. By roasting the copper mineral, we obtained copper(II) oxide. This new sample came out of the crucible grayish-black

manipulate the state of copper by taking copper through four different forms and to observe and understand the method behind each reaction. The transformations include starting from 0.1588g of Copper(II) Chloride dihydrate to produce Copper(II) hydroxide. Copper(II) Chloride dihydrate was dissolved in water forming a light blue colour and Sodium hydroxide was added in order to form Copper(II) hydroxide a dark blue precipitate. In this reaction Sodium Chloride is soluble and Copper hydroxide is insoluble

Following the formation of solid copper (II) hydroxide (Cu(OH)2), the solution was heated in order to break the bonds in the copper (II) hydroxide to form copper (II) oxide (CuO) and water (H2O); classifying this process as a decomposition reaction because the reactant was broken down into smaller compounds. While heating the solution, the opaque royal blue color became a clear colorless solution; furthermore, as the solution became clear charcoal color solution began to appear in the solution. The