Conclusion: This experiment was successful. Some possiblesources of error could have been in the thermometers not being accurately read, theheat lost to the air was not factored in, also possibly altering the results. Copper will undergo many types of reactions and go through its whole cycle, then return to solid copper to be weighed. Report this Essay; Save Paper. Use a spatula to add some copper chloride dehydrate to the beaker filled with water. The ascorbic acid is white inn color and is powdery.
The Copper Cycle Alexes Montalvo Chem 1500-10 September 26, 2012 The Copper Cycle Introduction: 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. In our lab, we made sure to wear closed-toed shoes as well as goggles at all times. The copper solid reacted with zinc, and then was washed with distilled water. Rope of Sodium Hydroxide, Noah, into copper-containing I Greenish- blue crystals forming, misty, cloudy, liquid. When all the liquids evaporated, I scraped off the solid and.
These reactions were conducted to display the several different states of… 1616 Words 7 Pages The Copper Basin of southeastern Tennessee is an area that is climatically unique with a rich history rooted in copper mining. Rinse the first beaker thoroughly and pour the rinse with the solution in the 250 ml beaker. We used a pipette to remove the excess water and impurities that were underneath the banana oil. I heated the solution to evaporate the water and I got a brownish-blackish solid called copper oxide. Classifying Chemical Reactions Through Copper Reactions. From 1837 to 1857, the penny was bronze; containing 95% copper and 5% zinc and tin. As we had our final solution of banana oil, we used the I.
While waiting for the mixture to cool prepare a suction filtration set. Stir the contents in the beaker with the thermometer that is provided. Copper is a metallic metal. In conclusion my percent recovery of copper was 100% due to the adequate amounts of solutions and achievement of proper chemical reactions. Defiance County is also an equal opportunity employer.
When the final mass of copper was weighed, the balance may have not been calibrated correctly, and the copper in the evaporating dish may have contained impurities, such as un-reacted zinc, that changed the mass that was measured. The initial mass of copper was recorded, and then compared with the mass of recovered copper at the end of the experiment. The primary source of error is when we use vacuumfiltration process, the error could be produce because the pipes are not tightenedproperly or it is loose on the flask. I I until chemical reaction has occurred. Inthis lab, we will be transferring heat from a hot copper sample to a cool water sample. After adding the 1 mL of glucose to the benedict reagent the color of solution remain unchanged, that is, dark blue color. In addition, the crystals stick together.
To test this law, copper can be put through a cycle to test if the same mass of copper is present at the end of the cycle. After this knowledge was obtained, one can conclude that the zinc ions were washed out with the water during the final step. At different stages of the cycle, copper was present in different forms. Now You See It — Copper Cycle Lab The purpose of the lab is to discover what happens when someone executes a series of procedures, beginning with copper metal. Add 6 drops of Sodium Hydroxide, Noah aqua , to the 250 ml beaker until a precipitate is formed. This lab also displays how matter cannot be created nor destroyed in a chemical reaction.
When aqueous sodium hydroxide was put into the aqueous copper nitrate, copper hydroxide immediately crashed from the solution into a blue solid and it is in the beaker with aqueous sodium nitrate. However if we determine the mass of each element in the compound we will be able to get the true chemical formula. All calculations must be typed or written legibly. This brown gas was nitrogen dioxide as the balanced equation above shows. You must submit the complete set of original copies i. Another situation which was a source of error was during step 5 when the copper solution and water was heated so that the contents of the beaker would boil. There are also a number of unincorporated areas.
The first step of the lab was to measure 2 g of copper and place it in a beaker. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion Cu2+. In conclusion my percent recovery of copper was 100% due to the adequate amounts of solutions and achievement of proper chemical reactions. The value I calculated for copper in this lab wasvery close to the value of copper in the table of specific heat. When the solid was hot, it bubbled and popped until it cooled down. The solution was swirled until all of the copper had dissolved.
Before the boiling process, the volume of mixture was 100 mL but after the boiling it decreases to 75 mL. It is also used in brass and bronze as an alloying agent. Introduction The scientific law that was tested in this experiment is called the Law of Conservation of Mass. In 1857, it was 88% copper and 12% nickel… 665 Words 3 Pages Copper Copper is a mineral. In the last step of Part A, we use Zn dust to react with mixture to obtain copper metal but if any Zn dust is still unreacted then it can affect the yield of copper metal. Additional heating will help indicate a chemical reaction has occurred. In theory, the exact same amount of copper should have been recovered at the end of the experiment yielding a perfect 100% recovery, but that is usually not the case in lab situations.
The error could occur while measuring over the analytical balance as a little disturbance over the shelf can vary its values. Therefore, thecopper was started in a boiling water bath and a thermometer was used to measure thetemperature of the bath to a tenth of a degree Celsius. In the final reaction, solid zinc was added to aqueous copper sulfate. Concessions will not be made for technical difficulties. The data recorded was used to see the different changes involved with a piece of copper metal.