Cycle of copper reactions lab answers

The reaction series includes single replacement double replacement synthesis and decomposition reactions. To convert elemental copper into di erent copper compounds by a series of chemical reac-tions regenerating elemental copper at the end of the copper cycle.

Fe₂O₃ s 3CO g 2Fe s 3CO₂ g Fe³₂O²₃ 3C²O² 2Fe⁰.

Cycle of copper reactions lab answers. 4 HNO3aq Cu s CuNO32aq 2 H2O l 2 NO2g Observations. Almost immediately after adding the nitric acid the copper began to dissolve and release nitrogen dioxide in the form of dark orange steam and turned the solution a teal blue color. Post-Lab Lab 4 - A Cycle Of Chemical Reactions Of Copper A Cycle Of Chemical Reactions Of Copper Are you completing this experiment online.

Yes Part I Data 0500 Concentration of stock solution of copper II nitrate. M Volume of stock solution of copper II nitrate in ml. 2500 Part V Data 8953 Mass of weighing paper and dish for mass of.

A Cycle of Copper Reactions In this experiment you will begin with the element copper and carry out a series of chemical transformations in which you will see copper in other forms. The last reaction returns the copper to its original metallic form which you will recover and. This reaction is an example of a redox reaction.

Where aluminum is oxidized and copper is reduced. The copper is the oxidizing agent and the aluminum is the reducing agent. 0 2Aluminum is oxidized.

-Al Al 3 3e Copper is reduced. Cu 2e - Cu 0. The dissolution of copper metal requires a solution containing what.

Nitration ions and hydrogen ions. The balance equation of the dissolution of copper metal. Cus 4HNO3aq - CuNO32 aq 2NO2g 2H2Ol after you dissolve coper metal what are we doing.

Copper nitrate can be used to generate nitric acid by heating it until decomposition and passing the fumes directly into water. This method is similar to the last step in the Ostwald process. The equations are as follows.

2CuNO32 2CuO 4NO2 g O2 g NO2 H2O 2 HNO3 NO g Copper nitrate soaked splints of wood burn with. The Chemistry behind each step of the Copper Cycle. Chemistry The different copper species obtained in each part is shown in Equation 1 below.

Cus Part I Cu2aq Part II CuOH2s Part III CuOs Part IV Cu2aq Part V Cus blue Figure 1 below. When the reaction mixture is diluted with water the Cu2 ions are hydrated. Chemistry questions and answers.

Lab Tham Members Classifying Reactions in the Copper Cycle Report Sheet 1. Initial mass of copper 2. Mass of copper and evaporating dish 3.

Mass of evaporating dish 4. Mass of uncovered copper 5. Percent yield show calculations x lou 0498 0498 51097 thearetaal 50502 0295 0295 a 123 5923 6.

Describe the reaction between HNO3 and the Cu metal in your lab report. Dilute the resulting solution with about 10 mL of deionized water. Describe the appearance of the resulting solution containing Cu2 in your data table.

Chemistry - Precipitating CuOH2s with NaOHaq In Part II two reactions are carried out by adding NaOHaq. In the first reaction the hydroxide ions. By pouring acetone into the evaporating dish and then waiting a few class periods for the copper to dry there is no exact way to tell if the copper is completely dry.

This means that a bit of other elements from the various liquids could still be in the evaporating dish leading to a. The sequence begins with copper metal and ends with copper metal so it is called a cycle of copper reactions. Observations will be made for each reaction.

Since no copper is added or removed between the initial and final reaction steps copper can be quantitatively recovered. In other words to recover the same amount of copper metal that you started with this will require careful work. The success of the.

In the first reaction copper metal is oxidized by nitric acid to form copper II nitrate CuNO 3 2. It is then converted to copper II hydroxide CuOH 2 by reaction with base. When this compound is heated it is transformed to copper II oxide CuO.

Copper II oxide is then reacted with acid to form copper II sulfate CuSO 4. Finally the copper ions in the copper sulfate are reduced to copper metal. According to the Law of Conservation of Mass the mass of the products must equal the mass of the reactants so logically one would expect that if 2 g of copper was used to start the lab the lab would result in 2 g of copper.

Unfortunately that was not the case in this lab and the final mass of copper exceeded the initial mass by 4841g. In this laboratory experiment students will perform a series of reactions known as the copper cycle. The reaction series includes single replacement double replacement synthesis and decomposition reactions.

In each of two cycles students will complete a series of reactions that results in the final product regenerating the original starting material. This experiment should take one 80-minute session. Copper Cycle Lab Report 2117 Abstract In the Copper Cycle Lab we observed a sequence of aqueous reactions of solid copper and its reaction formed.

We first weighed the solid copper and then after going through the cycle of copper being a solid compound or in ionic form. The percent recovery at the end of the lab was 978. Intro The purpose of this experiment was to observe a sequence of.

Reactions begins and ends with copper metal so it is called a cycle of copper reactions. Because no copper is added or removed between the initial and final steps and because each reaction goes approximately to completion you should be able to recover almost all of the copper you started with if you are careful. This cycle of reactions i s.

To convert elemental copper into di erent copper compounds by a series of chemical reac-tions regenerating elemental copper at the end of the copper cycle. Overview of Task Good laboratory technique is necessary for the successful cycling of copper through a. Reactions in which electrons are transferred between reactants.

-Reactions where an element forms a compound or an element is produced from a compound are redox reactions. Fe₂O₃ s 3CO g 2Fe s 3CO₂ g Fe³₂O²₃ 3C²O² 2Fe⁰. Lab Experiment On The Copper Cycle.

A series of reactions that convert a piece of copper metal via several different copper- containing compounds back into its original elemental form will be observed. Copper wire was dissolved in nitric acid. NaOH was then added to the dissolved copper solution precipitating into Cu OH2.

Copper Cycle Lab Report Introduction. The purpose of this experiment was to convert copper wire into different states using a variety of methods including oxidation-reduction reactions and acid-base reactions. Then at the end of the cycle one should end up with solid elemental copper again which theoretically has the same mass as the original sample.

Chemistry 11 Copper Cycle Stoichiometry Assignment 1 Consider the reaction below which is the first step in the process of recycling copper. CuNO32aq 2NO2g 2H2Ol a If a student began the experiment with 0020g of copper metal what volume in mL of concentrated 158M HNO3 would be required to complete the reaction. This lab is designed around developing observation skills.

Introduction In this lab the procedure began with copper and the result was a copper-covered nickel. Despite all the materials used and steps taken our result was the same as our beginning. This is the Copper Cycle.

Despite the chemical changes and reactions which is when a. 3 Reaction 1 Cus 4HNO3aq CuNO32aq 2NO2g 2H2Ol Copper Nitric acid CopperIInitrate Nitrogen gas Dihydrogen monoxide 1 Type of reaction. Decomposition reaction Reaction 2 CuNO32aq 2NaOHaq CuOH2s 2NaNO3aq CopperIInitrate Sodium hydroxide Copper hydroxide Sodium nitrate 2 Type of reaction.

Double displacement reaction Reaction 3. The reaction of nitric acid and copper must be done in the back of a fume hood. The noxious and toxic NO 2 gas produced during the reaction must not be allowed to escape into the lab air.

Do not under any circumstances add nitric acid to the copper metal unless your beaker is in a fume hood.