we preformed this experiment in a lab and the conditions were not perfect it was impossible to obtain the correct theoretical yield, that we expect when we combine the two reagents. Because of this the weight of the Cu3(PO4)2 that we get in the lab is called the actual…
In accordance with the procedures carried out in the experiment, the stated hypothesis was not entirely valid due to the changes in measurements. Aside from these changes, as their effect on the hypothesis and experiment is unknown, the hypothesis was rejected. The hypothesis stated that the yield of copper would be at least 25% less than the theoretical yield, though the data shows otherwise; the theoretical yield, as seen in the graph and calculations, was equal to .508 grams of copper product. This was calculated by taking the moles of copper found from the limiting reactant, the copper (II) sulfate pentahydrate solution, and placing it inside the n=m/M equation. This equation is used to calculate the number of moles but can be used reversibly to find the amount of grams by including the molar mass in…
The objective of this lab was to identify the limiting reactant, which the lab's data showed the limiting reactant to be Beaker A. According to the Limiting Reactant Document, it states "limiting reactants control the amount of product possible for a process because once the limiting reactant has been consumed, no further reaction can occur"(2nd paragraph). The mole of Beaker A was .00500 of CuCl2 as Beaker B's was .0056 mol of CuCl2. During the lab, Beaker A's solution had a larger amount of aluminum foil pieces than Beaker B's solution; showing that the limiting reaction has to have a smaller volume. In the Limiting Reactant Document, based on their second experiment, " Substance A and B react in a 1:1 ration, and with only 0.5 mol of Substance…
The purpose of this lab was to determine the formula of copper chloride hydrate by dehydration through heating, rehydration through adding water back in, the reaction of aluminum with the copper chloride hydrate to produce solid copper, and the weight of this copper. To accomplish this, a petri dish was weighed and 1.01 g of copper chloride hydrate was added to the dish. The solid salt crystals were broken up to make sure that all of the hydrate would be heated the same. Next, the petri dish and hydrate were heated upon a hot plate for roughly 15 minutes, until all the salt crystals were brown instead of blue. This indicated that all of the water had been burned out of the hydrate, leaving dehydrated copper chloride.…
Statement of Problem The Ely Copper Mine was declared a superfund site in 2001. Mining activity occurred from 1821 to 1920 Ore body discovered in 1813 Location The Ely Copper Mine is located in East Central Vermont in the rural town of Vershire, Orange County. The site is part of a region referred to as the Vermont Copper Belt, or the Orange Country copper district. Over 30 miles long, the belt runs in a NNE–SSW direction. The Ely Mine is one of three major mine sites in the region.…
Process To Make Copper Coated / Plated Nails 1) Measure out 1/4 cup white vinegar and put into the glass bowl. 2) Add 1 teaspoon salt. Stir salt until it dissolves in the vinegar. 3) Take a penny and submerge it into the vinegar solution 1/2 way for 10 seconds.…
In addition to time, the mass of the hydrated copper (II) sulfate is also more and contributes to the difference in mass and percent…
This experiments goal was to successfully produce ZnI2 by using Zinc Sulfate (Heptahydrate) and Barium Iodide Dehydrate, which Jessica and I did with acceptable success. The definition of acceptable success for this experiment is measured by how close our percent yield was close to the ranges provided (0-2% being considered excellent precision and etc). Our percent yield was 92 % meaning that it was an acceptable, but not exactly as close to what we wanted it to be. In order to try and figure out what the mistake was that caused us to get 92% we had to evaluate how well we did our experiment. We followed all the instructions as close as possible and double read the step that would come next.…
They will then attain five small test tubes, in which they will mix varying amounts of copper sulfate and sodium hydroxide. Once a precipitate has formed in all five test tubes they will record and analyze their observations. Fun Fact: The technique used to determine the limiting reagent in part A of this lab, is used to determine how much of a desired product can be produced, which is tremendously important in the medical field.…
In the experiment the percent of water and percent of copper can be calculated with the masses that were taken before and after the reaction. The calculations of the percent of water and copper are shown below: Water: 5H2O:(2.194g3.385 g)*100 64.814% Copper: Cu:(1.104 g3.385 g)*100 32.614% When finding the theoretical percent of water and copper one can find the molar mass of each and find the percent. The calculations are shown below: Water: 5H2O:(90 g153.546 g)*100 58.614% Copper: Cu:(63.546 g153.546 g)*100 41.356% Analysis of results…
Sarah Bounab BQD Experiment 2: Copper/Iron Stoichiometry Abstract: The purpose of the Copper/Iron Stoichiometry lab was to determine which of the two possible iron sulfate compounds formed when reacting aqueous copper(II)sulfate with solid iron metal. The techniques used in this lab were weighing by difference, quantitative transfer, and vacuum filtration. At the end of the experiment it was found that iron was the limiting reactant and iron(II)sulfate was a product of the reaction between 7.0002g of copper(II)sulfate and 2.0101g iron metal which produced 2.3037g of copper product with a percent yield of 100.72%.…
Data Calculated from Experiment Solid-Liquid Weight (g) Solid-Liquid % Recovery Liquid-Liquid Weight (g) Liquid-Liquid % Recovery Acid 0.01 20 % 0.028 56 % Phenol 0.011 22 % 0.001…
By measuring out two grams of our unknown, and heating it up until the difference of the mass of the test tube and the anhydrous residue subtracted to 0.002g, we were able to calculate the percent water in the two possible unknowns, and then our unknown, to figure out which unknown we were given. Since our percent water was 44.9%, we concluded that our unknown is Zinc Sulfate. A possible error as to why our calculated percent water was not exact to the theoretical percent water was most likely because we did not measure exactly two grams of the unknown. Our percent error was 2.5 % due to the mass that we measured in the beginning of this experiment. Finding unknowns is very crucial to chemistry because if there is a problem, for example, of…
In this experiment my partner and I will set up a chemical system arrangement in order to determine the effectiveness of neutralizing of a commercial antacid, per gram. When the arrangement is set we will test the different variations of the experiment, for example during step A we will be my partner and I will be determining the mass of the antacid and preparing the antacid for analysis. For step C my partner and I will be using what we have recorded in order to complete the calculations. Another reason for conducting this experiment is too figure what kind of solution will form when the antacid is dissolved.…
Purpose: The purpose of this laboratory was to synthesize isopentyl acetate, commonly known as banana oil, in a reaction of methanol and isopentyl alcohol catalyzed by sulfuric acid. Through this Fischer esterification reaction, it was possible to learn about using a Reflux condenser to run a reaction as well as purifying the product through various washes and extractions along with simple distillation. In addition, the product of the experiment was carefully analyzed based upon boiling point, physical characteristics, IR and 1H NMR. The overall objective was to successfully isolate the product of isopentyl acetate and observe the purity of this product.…