Chemical Reactions Lab

6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__

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 objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

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

Substances A and B have an appearance of a white solid like. Substances A and B were put into a test tube and on the Bunsen burner. As a result, B melted faster than A. A was slow to melt. The reason why B melted faster than A is because it has a lower boiling point than substance A which made it melt faster. It also shows that A needs more energy than B to be broken down.

In this lab we will be heating up substances and use them to galvanize pennies. When you heat up the zinc, and then coat the penny in it, it then galvanizes the penny. Meaning, it helps protect the penny from oxygen and water. Afterwards, you will need to record data such as the mass of the penny. This helps keep track of what physical traits are being changed during this experiment. On part B of this experiment, you will be heating up the now galvanized pennies in order to see what reaction you get. The reaction you should receive from heating up the now zinc-covered pennies is that the pennies will change color.

Procedure: In the first experiment (Synthesis Reaction) 5g of Mg was heated with a Bunson burner to perform a reaction. In the second experiment (Decomposition Reaction) 5g of Cu2Co3 was heated with a Bunson burner to perform a chemical reaction with visible physical properties. In experiment 3 (Single Displacement Reaction) 15 mL of 6 M hydrochloric acid (HCl) was put into a Erlenmeyer flask and was stopped with an airtight stopper to record the temperature and pressure when .25g of Zinc was added. In Experiment 4 (Double Displacement Reaction) two separate beakers were used. In the first one there was 15mL of NaOH and the second contained NiCl2. These were poured into each other to watch what reaction would take place.

A hot plate was placed on a ring stand with a 50 mL beaker being placed on a hot plate. The ring on the ring stand was positioned to surround the beaker. Rubber tubing, a funnel, and an aspirator was then used to make an aspirator, with the funnel placed over the beaker connected to the aspirator. The HNO3 used in Step 1 will give off toxic gas, which the funnel will prevent from spreading away from the beaker. 250 mg of copper was weighed and transferred into the 50 mL beaker. 5 mL of M HNO3 was poured into a 10 mL graduated cylinder. The aspirator was turned on by starting the water and 4 mL of HNO3 was added to the beaker and slowly heated with the hot plate. After the reaction occurred the aspirator was turned off and 10 mL of distilled water was added to the beaker. 6 M NaOH was added in drops to the solution and stirred with a stir rod while periodically

During this particular lab there were various chemical reactions that we had to observe and describe with much detail. In “Part One” of the lab we continued to mix various substances, and then noted descriptive characteristics such as smell and color. This particular portion of the lab was interesting because each mixture lead to a unique reaction. For example, after we mixed the substances “E” and “F” the final substance smelled similar to wood, but this did not occur in any of the other final solutions. Therefore, this part of the lab allowed us to experience a wide range of chemical reactions, which caused an assortment of changes. This aspect of the lab does need to be improved because it was an insightful experiment that forced each student

The zinc and sodium hydroxide solution, when heated formed sodium zincate* (Na2ZnO2) which when introduced to the copper penny the zincate ions (ZnO2-2) in the solution to bind to the copper of the penny, after a minute it gets reduced to metallic zinc that coats the penny. This process involved a chemical change as the sodium zincate formed, and a physical change as it coated the penny, a new substance was not formed. When the penny was heated over the bunsen burner flame the zinc and copper combine to form the metallic mixture brass. This process was a chemical change as the copper and zinc melted together to form a new substance. Copper is a substitutional alloy, meaning that because the elements Zinc and Copper are close to each other on the periodic table, they are similar in size and can easily exchange atoms (zinc gives to copper). We could have tested whether or not the substance was gold by measuring the density of the penny, or by applying nitric acid to the penny and looking for signs of oxidization, but it was easy to observe that there was no miraculous change from copper to gold. In conclusion, my hypothesis that the pennies wouldn't turn into gold, but rather a copper alloy was correct. The substance actually created was not gold but brass, a copper and zinc

First we added 4 mL of HNO3 into a beaker. After the substance dissolved, distilled water was added until the beaker the beaker was half full. The mixture was then stirred into the distilled water. Add 30 mL of NaOH into the solution, and stir. The solution was then heated slow. As the product was heating slowly it was stirred. A thermoter was placed on a ringstand and clamp and then placed inside the solution.The solution was heated until 61 degrees celsius. The beaker was then removed from the heat and left to settle. 200 mL of distilled water was placed inside a 400 mL beaker and put on the heater. When the CuO settled for 10 minutes, the solution was then placed inside of a funnel. After the solution is drained, the copper is then washed away with the distilled water. The soultion was tested with a litmius paper. 15 mL of 6.0 mL of H2So4 into the solution. Next the Zinc must be added, then observe the reaction. Then add 10 mL of 6 M Hcl to the Cu. Pour out the Hcl, then add water to the copper and rinse. Then get a beaker and add Cu to water and apply heat.

The experiment was divided into two parts. Part A was to recover the copper metal using the copper cycle method and part B was to observed copper (I) compounds. Every copper complexes and compounds indicated in the experiment was observed very carefully. Any chemical changes in each step were recorded at instant. Such as, In Part B copper (II) nitrate was combined with sodium hydroxide to form an light blue precipitate of copper (II) hydroxide which upon heating, gives us a black colored precipitate of Copper (II) oxide.

In relation to this experiment, the per cent recovery, or “how much of the original pure copper mass recovered at the end of the experiment”ii iii iv v should be 100% because all of the copper should return to elemental form. However, the per cent recovery from this experiment was calculated to be 56.5% recovery, much lower than the anticipated value, and therefore does not appear to support the Law of the Conservation of Mass. One explanation for the per cent recovery being too low would be that some copper was lost while decanting the solution after reaction three. The time constraints also should be taken into consideration, as if the reaction resulting in the precipitation of copper by the aluminium wire was allowed to run longer, more of the copper could have been precipitated out of solution, closing the gap toward the 100% recovery. The product of the reaction was a dark reddish brown colour.

Powdered zinc 3. Balance 4. 2 Test tube 5. 1M Hydrochloric acid (approx. 20 ml)

Cloudy at the bottom of the test tube. Cu2+ Solution changed to a light blue, water consistency White dust accumulated at the bottom of test tube, surrounded by watery consistency with shades of sunset orange and yellow throughout Precipitate formed with a light blue color, small separation in the liquid with no change in color. Separation occurred closer to the bottom of the test tube. Fe3+ No reaction Initially burnt orange, more clear color toward the bottom of the test tube.