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Single Replacement Reactions Lab Report

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Reactivity of Metals in Single-Replacement Reactions

A lab was conducted to test the reactivity of metals in single-replacement reactions. This lab was done to solve the problem of which metals will replace each other in single-replacement reactions. A single replacement reaction is a type of oxidation-reduction chemical reaction when an element or ion moves out of one compound and into another. It was presumed before the experiment that the location of the metal on the Activity Series chart would thus determine the reactivity of the metal. Copper, magnesium, iron, and zinc were all tested in the same five solution compounds; which included hydrochloric acid, sulfate, magnesium chloride, iron chloride, and zinc chloride. Observations of chemical changes within the reaction were recorded to describe the results of the reaction and each metal's reactivity. An example of a single replacement reaction is the Statue of Liberty, which has copper on the outside and iron as an inner support. As time went by, the copper started to react with air and form a verdigris coat, or a bright bluish-green patina. Meanwhile, a single replacement reaction between iron and verdigris takes place so that Verdigris on the outside is replaced back to copper but the iron support is oxidized and rusted. As a result of this reaction, approximately 1800 iron …show more content…

The same metal was placed in vertical columns in an effort to organize the metals. Groups moved to each solution labeled and covered the metal in the respective solution. Observations to how each metal reacted to a solution were then recorded. Each metal was covered in five different solution compounds. Unless the metal and the solution compound contained the same element, such as iron and iron (III) chloride. To cover this metal in this solution would have been counter productive since the same product would have been

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While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.

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An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

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PURPOSE The purpose of this experiment is to conduct a single displacement reaction using a reactant with impurities to deduce its effects on the actual yield of the precipitate by calculating percentage yield. INTRODUCTION In chemical reactions, there are limiting reagents which control the maximum yield of products. On the other hand, excess reactants are other reactants in a reaction that are left over or remain after the limiting reagent has been completely consumed.

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Consequently, it induces second element to be oxidized. 2. In the experiment #3, zinc electrode acts as anode, where the oxidation processes occur, while iron half-cell acts as cathode, where the reduction processes appear. In the experiment #4, iron is visa verse reducing agent that evicts electrons to copper half-cell through the circuit.

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1366 Words | 6 Pages

Then more roasting occurred when the crucible was placed into a ceramic triangle for the Bunsen burner to continue its burning for an additional 90 minutes. Once the burning was officially over, the crucible was placed onto a ceramic tile to cool off. Next the charcoal and copper material were poured onto a paper towel and were separated from carefully distinguishing them one from the other. Then comparisons were down through analysis of the copper (II) oxide smelted.

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Nucleophilic Substitution: Preparation of 1-Bromobutane and Alkyl Halide Classification Tests Introduction This procedure was undertaken in order to convert a primary alcohol, 1-butanol, into a primary alkyl halide, 1-bromobutane. This was done using hydrobromic acid. Additionally, tests were performed to assess the degree of the alkyl halide: primary, secondary or tertiary.

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This process forms a zinc coating producing a corrosion resistant. However, A corrosion resistant is a multi-layered coating of zinc –iron alloy and zinc metal. During the galvanization process a metallurgical reaction occurs. A metallurgical reaction is a diffusion process so the coating forms perpendicular to all surfaces.

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Evidence of such loss of material was displayed as a white film on the end of the tongs which held the metal. If the reaction was conducted in a more controlled environment, then maybe the theoretical results would be

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Experiment 2 Report Scaffold (Substitution Reactions, Purification, and Identification) Purpose/Introduction 1. A Sn2 reaction was conducted; this involved benzyl bromide, sodium hydroxide, an unknown compound and ethanol through reflux technique, mel-temp recordings, recrystallization, and analysis of TLC plates. 2. There was one unknown compound in the reaction that was later discovered after a series of techniques described above.

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Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and

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As soon as the wire was submerged into the solution, the aluminum atoms and the copper (II) ions underwent a reduction-oxidation (redox) reaction, meaning aluminum was oxidized and donated its electrons to the copper ions, which were reduced. As a result, solid copper began to form on the surface of the aluminum wire, giving the wire a brown-orange color that resembled rust. The wire had to be regularly shaken in order to remove the solid copper particles and thereby expose more of the aluminum wire to react with the surrounding solution. As the reaction progressed, the liquid copper chloride solution slowly began to lose its color and turn clear. This was a chemical reaction, as seen by the bubbles formed with the wire was added, meaning gas was released when aluminum was oxidized and copper was reduced, but it also gave rise to physical changes, such as the change in color of the solution from blue-green to rusty orange to clear.

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Introduction: The purpose of this experiment is to demonstrate the different types of chemical reactions, those including Copper. There are different types of chemical reactions. A double displacement reaction is a chemical process involving the exchange of bonds between two reacting chemical species. A a decomposition reaction is the separation of a chemical compound into elements or simpler compounds and the single-displacement reaction is a type of

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The purpose of this experiment was to learn about the electrophilic aromatic substitution reactions that take place on benzene, and how the presence of substituents in the ring affect the orientation of the incoming electrophile. Using acetanilide, as the starting material, glacial acetic acid, sulfuric acid, and nitric acid were mixed and stirred to produce p-nitroacetanilide. In a 125 mL Erlenmeyer flask, 3.305 g of acetanilide were allowed to mix with 5.0 mL of glacial acetic acid. This mixture was warmed in a hot plate with constantly stirring at a lukewarm temperature so as to avoid excess heating. If this happens, the mixture boils and it would be necessary to start the experiment all over again.

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The final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.

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1645 Words | 7 Pages

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