Sequencing Copper Chemical Reactions Lab Report

It is a chemical reaction where the colors of both solution and iron strip changed. It is

The objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

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

3. Find the number of atoms of each of the substances involved in the 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

-If the copper metal is submerged in the silver nitrate solution then in reaction, a pure, solid (Ag) silver product is created with an excess of (Cu (NO3)2) copper (II) aqueous liquid because a single displacement reaction occurs where the balance equation is then

Copper starts to dissolve and bubbling occurs when nitric acid was added. The solution became green and the beaker started to become orange/brown as gas was being released. Solution then became light blue when washed with water.

The Oxidation of a Secondary Alcohol with Sodium Hypochlorite experiment was performed to show how to change an unknown alcohol into a ketone. The unknown that was found for this experiment was Compound A. Once the ketone was found from the unknown alcohol, an IR and the boiling point was taken to try and figure out what the product and starting alcohol actually is. The first thing that is added to the 1.50 g of unknown compound A is 15 mL of 8.25% of NaOCl, which is a bleach solution. This reacted with the alcohol so the solution could then be tested using the iodide-starch paper. The reaction came out positive when tested because a blue, black spot appeared on the strip.

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.

I started with elemental copper metal and then reactions occur step by step as follows:

Experimental approach: In the first reaction, copper metal turnings oxidize when put in contact with nitric acid and become copper nitrate.

Copper Equation: Cu2+ + 2OH- Cu(OH)2 Sodium hydroxide test – few drops of sodium hydroxide are added to a solution of a metal compound. Light blue precipitate is formed Nickel Equation: Ni(s) + 2H+(aq) + SO42-(aq)  Ni2+(aq) + SO42-(aq)

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:-

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the

At the end of the experiment when the lid was removed, it was found out that the blue colour of the copper (II) sulphate solution has faded away. It was turned to pale grey and there were some precipitates present. It was the zinc powder that was in excess to ensure that the copper (II) sulphate solution could react fully with the zinc powder.