Double Displacement Reaction Lab Report

The main objective of this experiment is to differentiate between a physical change and a chemical change.

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

When the zinc was dropped in the hydrochloric acid, the substance began bubbling vigorously, forming a precipitate. Eventually, the zinc dissolved completely. After the lit wooden splint broke the surface of the test tube, there was a loud popping noise. The gas that was released was hydrogen from the acid and the popping noise was a result of the Hydrogen being burned up by the fire creating a small explosion. Two chemical changes occurred in this test: one with the formation of a precipitate (a textbook sign of a chemical change), and the other when the explosion

11. Write the balanced chemical reaction of zinc with HCl (same as problem 5). Is the product of

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

-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

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

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:-

When predicting products in a double displacement reaction, we need to identify the different ions first and their charges. After that, we switch the ions of the two reactants and write down the products. The final step is to make sure that your chemical equation is balanced. There are three types of reactions that fall under the double displacement reaction category: precipitation, gas formation and neutralization reactions. A __precipitation reaction__ forms an insoluble solid compound.

The change in colour of the copper wire from bronze to black signifies that the composition of the copper wire have changed during the heating process. The copper wire, Cu had reacted with oxygen, O2 during heating and forms a new substance that is copper oxide, CuO. As the composition of the copper changes with the presence of oxygen, the chemical properties have also changed and thus this causes the resulting substance, copper oxide, CuO to differ physically and chemically with the original substance, Copper, C. Thus, it can be concluded that the heating of copper wire causes a chemical change to occur. Meanwhile, the change in physical state and colour of the iodine crystals, I2 during heating does not signify that a chemical change has taken place.

The nine different metal ions, aluminum, barium, cobalt, copper, iron, magnesium, manganese, lead and zinc, were reacted with sulfate, iodide, carbonate, hydroxide, and ammonia. When reacted with sulfate aluminum, cobalt, copper, iron, magnesium, manganese, and zinc all had no reaction. Barium and lead both formed white precipitates. When reacted with iodide aluminum, barium, cobalt, magnesium, manganese, and zinc all had no reaction.

There are two types of displacement reactions : One type is called the single displacement reaction, the other is called the double displacement reaction. During a single displacement reaction, an element substitutes another element in a compound, creating a new element and a new compound as products. In most single displacement reactions, either a metal replaces another metal, or a non-metal replaces another non-metal. The more reactive element takes the place of the less reactive element in the compound, otherwise the reaction will not occur. The general chemical equations of single displacement can be: A (metal) + BC → AC + B,

Elemental copper underwent five chemical reactions before cycling back to elemental copper. Reaction 1 was an oxidation-reduction reaction. Elemental copper was mixed with concentrated nitric acid and the solution went through several color changes as the copper reacted with the nitrate ions. The nitrate ion oxidized the copper metal to a copper(II) ion and transformed to nitrogen dioxide in the process. This reaction was

Excess nitric acid was still present in the solution and reacted with the strong base of NaOH in order for the solution to be neutralised. The excess NaOH allowed a double displacement or metathesis reaction to occur. This was where the copper (II) ions react with the OH- ions to produce an absolute blue precipitate of copper hydroxide which was insoluble. Sodium nitrate however is soluble in water and thus stayed dissolved in the solution (4). The insoluble blue precipitate observed in the reaction is supported by this explanation.