Reactivity Series Lab

The main goal of this experiment was to observe series of reactions that convert a piece of copper metal, via several different copper-containing compounds, back into its original elemental form. The data collected was the striking color changes along with their relevant chemical equations. The data was collected while keeping a close eye on the experiment the whole time. The data recorded was used to see the different changes involved with a piece of copper metal. The copper was weighed and heated multiple times throughout the experiment

The reaction between Copper (II) Chloride and aluminum has a formula that follows this basic single replacement formula. Aluminum was able to replace copper during the reaction because it is higher on the activity series. If aluminum

this experiment had a similar scenario to part A except the metals were switched and replaced with

b) Iron and Barium were present in unknown 3. Assigned unknown reacted with all 4 reactants and formed precipitate with 3 of them (Sodium carbonate, sodium hydroxide and Sulfuric acid). During the experiment it reacted very similarly to Iron (III) nitrate and Barium nitrate. For example, with it was tested against Ammonium Chloride, the color of the solution changed to a light green, very identically to Iron (III) nitrate and Ammonium Chloride. Besides, unknown 3 formed an orange brownish precipitate when it was tested with sodium carbonate. Iron (III) nitrate acted similarly. Moreover, unknown 3 reacted similar to Barium nitrate when it was tested against ammonium chloride and sulfuric acid. It did not form any precipitate with ammonium chloride but formed a very light white precipitate, which is identical to barium nitrate’s reaction against sulfuric acid. Therefore, the two present metal in unknown 3 are Iron and barium.

Therefore the more active element takes over, the equation changes, and a reaction takes place. The fourth reaction, zinc and hydrochloric acid, produced a gas, hydrogen gas. The final test was between copper and hydrochloric acid, which resulted in no reaction. Nothing occurred because the hydrogen is more active than the copper, thus the solution does not change. This lab was successful in showing the effect of a chemical reaction and how single replacement reactions

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

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 Relationship between Reactants and Products Results and Discussion The starting material of the Calcium chloride (CaCl2) was varied with each of the five Erlenmeyer flasks, while the Sodium carbonate (Na2CO3) remained unchanged through the reaction according to the Lab Manual.1The reaction of Calcium chloride and Sodium carbonate in each of the Erlenmeyer flasks that occurred resulted in a cloudy blue and white mixture. Once the mixture was added into the suction filtration system created, a powder like solid formed on the filter paper that was a part of the Buchner funnel. Tufts University School of Medicine did an experiment with a Buchner funnel and agreeably finds the funnel satisfactory.2 In this way, the suction filtration is being

In this lab there was a performance of a single replacement chemical reaction. The reactants of the reaction was solid iron metal, and copper (II) sulfate solution. This was a gravimetric lab and therefore it was crucial to begin by massing the reactants individually. The copper (II) sulfate was initially a solid. A procedure was conducted to dissolve the copper (II) solid by heating it in water to create the necessary solution. Once that was complete the following action was to react the solid iron and the copper (II) sulfate solution. The single replacement chemical reaction took place and there was a replacement of copper with iron. The products of the reaction was solid copper metal and an iron (II) sulfate solution. The solid copper was

All elements had a reaction but potassium had a greater more rapid reaction than the others. This indicates that elements that are lower in the periodic group will have a faster and greater reaction. This is due to its decreased electronegativity where it is easier for that element to lose its valence electron and hence having a faster and greater reaction, as the last elements in group 1 have a greater atomic radius than the beginning elements of group 1. In all elements there was a reaction which created hydrogen gas and made a solution that was alkaline. All the elements dissolved and turned the water purple; this indicates that all the elements tested are base, Alkali metals elements.

Materials: 4 test tubes 1 dropper 1 test tube rack Safety goggles Sodium chloride Sodium bromide Potassium iodide Unknown substances A, B or C Hydrogen peroxide Ammonia silver nitrate Nitric acid Sodium thiosulfate Potassium permanganate Method: Please refer to SCH3U Learning Guide 6- Periodic Table “Comparison of the Behaviour of Halides” worksheet.

To know if there was a reaction there was seen a color change of the metal of one or multiple of the following a conduction of heat, and fizzing or bubbling. For the reactions that was seen there was (Zn+FeNO3 = Fe+ZnNO3), (Mg+FeNO3 = Fe+MgNO3), (Mg+CuNO3 = Cu+MgNO3), (Mg+PbNO3 = Pb+MgNO3), (Pb+ZnNO3 = Zn+PbNO3), (Pb+CuNO3= Cu+PbNO3). There should have been ten different reactions but the data that was collected was turned up was six, here are the other reactions that should have

Virtual Lab: Developing a Metal Activity Series Purpose: To develop a metal activity series based on a series of potential metal and aqueous solution reactions. Procedure: The virtual lab was accessed by clicking on the following link. The student was directed to another page where they performed some virtual reactions between metal strips and aqueous salts and acids.

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

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