Abstract The main goal of this lab was to find the percent yield of a chemical reaction in which copper (II) chloride and sodium carbonate react to make copper (II) carbonate and sodium chloride. A solution of sodium carbonate and copper (II) chloride solutions were mixed to start the reaction. Then, a paper filter had to be used to separate the copper (II) carbonate precipitate from the rest of the mixture. The experiment determined the actual percent yield of 77.2%. Introduction:
Copper Transformations Prelab Questions Three metals ions are Magnesium, Iron, and Nickel. Iron is used in the sea with iron rich minerals, for substances. Iron was also used in the formation of earth.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
Once the material was acquired, 1.0094 grams of Aluminum were weighed and then transferred to a 250mL beaker. The 250mL beaker continued to remain in use for the next few steps. 1.4M KOH solution was added to the Aluminum sample that was previously obtained. For gas to escape the lab, there was a fume
The % yield was greater than 100% because the actual yield was greater than the theoretical yield. One error that may have caused this result to occur was that the copper may have not completely dried over the time it was left. If water was still inside the copper, it would increase the mass of the actual yield. If the copper was left in the beaker to dry for a longer time, it would help decrease the mass of the copper (as the water would be completely dried out) and bring the actual yield down.
In this experiment, aluminum is converted into potassium aluminum sulfate, or what the paper will now refer to as “alum” in order to see how much of the can is recyclable. The purpose of the abstract will be to go over the process of producing alum, writing net ionic equations for each step in the production of alum, and calculating the percent yield of alum. Materials and Methods The first step was adding 1.1013 g of aluminum can pieces to a 250. mL beaker.
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
The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.
To better understand this law, Cu(s) was transformed with different reactions only to return back to Cu s). The initial and final mass of Cu(s) was recorded to give the percent recovery of copper product at
Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.
In a Scenario like this I would direct everybody to the lab quietly without making any noise. Once we arrive to the lab my best friend will lock all doors as the professor and I start to look for metal bars,bubble wrap, masks, goggles, and scissors. Once we've found the materials I'll give everybody a roll of bubble wrap to wrap themselves with just incase the zombie bites them it wouldn't hit their flesh. Then they would put on the mask and goggles just in case the zombies' blood splash, it wouldn't get in their mouth, eyes or other openings. The metal bar is going to be the best tool to stab the zombie in the head with but the scissors will be there as a back up tool. Once everybody is ready my best friend will
Abstract In this experiment the separation of a copper (II) chloride and sodium chloride mixiture was attempted. The main aim was to separate the compounds from eachother while receiving as much of the original mass of both substances as possible - in perfect conditions the original mass will be received after seperation. Many techniques were considered but dissolution, filtration and evaporation proved to be easiest and most reliable in a school environment with school equipment. The copper (II) chloride and sodium chloride mixture was dissolved in a methanol solution and filtered out leaving the sodium chloride behind.
A foil is most commonly defined as a character who contrasts with another character. Foils are all around you, yet they usually go unnoticed. The Wicked Witch and Glinda the Good Witch. Peter Pan and Captain Hook. Shrek and Donkey.
Purpose This experiment is to determine the concentration of the solute copper sulfate pentahydrate, and the unknown solution, by passing different wavelengths of light through each solution. Procedure Weigh out approximately 5g of copper sulfate pentahydrate. Record the mass and place the solute into a 50 mL volumetric flask. Fill half of the flask with distilled water, add the stopper for the flask, and lightly shake the flask, until the copper sulfate pentahydrate fully dissolved.
The materials I used for this experiment were foam, duct tape, tin foil, yarn, cardboard, and a tin can. My idea came from the idea of a cooler because of the inside foam insulation. I got the idea of the duct tape when I thought about air ducts and how they wrap them in duct tape to repair them, and how you can't feel the heat from the ducts. I got the Idea for the tin foil, because tin foil is used for baking. I got the idea for the yarn because I thought it would be good insulation for a top because cotton is a good insulator and cotton is like yarn.
