Metallic Copper Lab

The purpose of this lab was to determine the empirical formula of copper oxide compound. In the lab, hydrochloric acid and copper oxide compound was mixed until it formed a blue solution. An oxidation-reduction reaction, a reaction in which there is an exchange of electrons between elements, was performed by adding zinc to the solution to displace the copper in copper chloride. Zinc, in this case, was oxidized by losing two electrons (0 → 2+) while copper was reduced by gaining two electrons (2+ → 0). Also, when the copper was displaced, it became a precipitate, which is a substance that comes out of a solution as a solid due to insolubility.

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

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 purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

Product bubbled upon addition to the hydrochloric acid; liquid turned cloudy ¡V precipitate was present; zinc sample disintegrated slowly and turned black in color.

In this experiment, the solid copper metal was weighed to get the initial mass to later compare the mass to the copper after all the reactions. The copper was put into a 250 ml beaker under the fume hood in order to measure excess amounts of 15.8 M nitric acid, HNO3 because the copper has to be the limiting reactant in order to change the state of matter of the copper. It needs to be aqueous instead of a solid. (Cu(s) + 4 HNO3 (aq) -> Cu(NO3)2 (aq) + 2 NO2 (g) + 2 H2O (aq)). After the reactants have reacted, 25 mL of water was added to the beaker to dilute the dangerous acid in the beaker for safety. Then 4 squirts of potassium hydroxide, KOH, was added to react with what’s now in the beaker, Cu(NO3), and this caused another reaction to happen (Cu(NO3)2 (aq) + 2 KOH (aq) -> Cu(OH)2 (s) + 2 KOH3 (aq)). Now the

-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

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

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:-

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:

This section of the experiment was composed of a series of different chemical reactions. In the first reaction, a small piece of zinc is placed is in a test tube that contains 2 mL of 6 M HCl; observations were then recorded. The next reaction, which should take place under a hood, requires a 1-inch copper wire to be placed in a clean test. Concentrated nitric acid is then added and observations are recorded. In the third reaction, 1 mL of 0.1 M sodium oxalate, Na2C2O4, is placed in a clean test tube.

The reaction characteristics 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 (II) because of low pH (6.0) of the solution [12]. The copper content according to the reaction mole ratio were 57.7, 50.5, 58.8, 59.3, and 59.8 wt% at the reaction mole ratios of 1.20, 1.32, 1.44, 1.56, and 1.68, respectively.

When the zinc was added to the copper (II) sulfate solution, the solution started to bubble. As the solution was stirred, it turned a cloudy blue. Small flecks of a brown solid were visible. As the solution became colorless, the brown solid settled to the bottom of the beaker. The solid formed was copper in its elemental state. The color faded from the solution as the copper ions slowly formed into solid copper. The copper was poured into a funnel with filter paper and washed three times with 25 mL

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.