An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the
In order to begin this experiment, first one must find the balanced chemical equation for the reaction which occurs between the aluminum and copper (II) chloride. This balanced equation being 2Al(s)+3CuCl2 (aq)3Cu(s)+2AlCl3 (aq). After finding this equation, one must use the process of stoichiometry in order to find how many grams of aluminum are needed in order to produce 0.15 grams of copper. In this experiment, the purpose was to produce between 0.1 and 0.2 grams of copper, so one should attempt to produce 0.15 grams of copper seeing as it is the average of those two numbers. The first step in the stoichiometric process which one has to complete is finding how many grams of copper are in one mole of copper.
Lab 27. Stoichiometry and Chemical Reactions Report In our lab we were asked Which Balanced Chemical Equation Best Represents the Thermal Decomposition of Sodium Bicarbonate. Sodium Bicarbonate is a chemical compound with the formula NaHCO3, also known as baking soda. In the process to answer our guiding question we have to determine how atoms are rearranged during a chemical reaction.
Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g). The decomposition reaction was performed in a crucible and heated with a Bunsen burner.
The elements needed for calcium carbonate precipitation (CaCO3) are calcium, carbon and oxygen which is present in the table 2 shows the elements present in the soil being tested in the scanning electron microscope (SEM). Carbon has a total mass percentage of 16.1, oxygen has a total mass percentage of 12.16, and Calcium has a total mass percentage of 2.46. Calcium carbonate (CaCO3) is an important chemical compound made up of one atom of calcium (Ca) bonded to one atom of carbon (C) and three atoms of oxygen (O). Its molecular formula is (CaCO3). It only proves that calcium carbonate (CaCO3) precipitation occurred in the soil because of the Bio-Vege
Because carbon dioxide is absorbed by the plant during photosynthesis less carbon dioxide present in the chamber is a sign that photosynthesis is working. The four lights used for this experiment range across the light spectrum on both sides in order to test a wider variety of wavelengths. All lights will be placed directly on the spinach leaf at the same distance so as not to give any spinach leaf a different light intensity, which could affect the data. This experiment will be able to show which light, ranging across the light spectrum, will allow the Spinach to perform photosynthesis more efficiently.
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%.
Stoichiometry of a Precipitation Reaction University Student Name Abstract The purpose of this experiment is to calculate the actual yield of Calcium carbonate from the reaction of Calcium Chloride with Sodium carbonate. We have to then compare the actual results with the theoretical value of Calcium carbonate and find out the error. When we mix 1.0 grams of Calcium Chloride and 0.80 g of sodium carbonate, it produces around 0.60 g calcium carbonate in the actual experiment.
After completing the lab, the actual data collected was not the same as the theoretical values. The theoretical yield was 2.75g of PbSO4, but the actual yield was 2.90g of PbSO4. A possible component that caused the error was the inaccurate weighing of the reactants. It is nearly impossible for someone to collect the exactly 3.00g of the given reactants. If exactly 3.00g of the reactants are not measured out, then it will cause an error in the experiment.
Finding the average mL NaOH added during the steep section of the curve. The mL are added together and then divided by the number of values used. Using stoichiometry to find the concentration of CH3COOH. The equation n =Cxv fis used to find the moles of NaOH, which can then be changed into moles of CH3COOH with a mole ratio The moles are converted into the concentration using C=n/V. Finding the concentration of H30+ by using initial pH of the equilibrium.
For determining certain molecules different techniques are available. To determine the presence of proteins in the Cobalt solution a spectrophotometer will be used to allow the proteins to interact with the light waves, this allows to measure the amount of light transmitted by the protein solution. To determine nucleic acids, adding indicators such as methylene blue, ethidium bromide, or diphenylamine will allow the nucleic acid to become visible. Also, benedict’s solution changes pigmentation of solution to indicate the presence of ions or sugars.
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 solution turned red when it reached the end point. The titration was continued for 10 seconds after a permanent red color was obtained. The volume of 0.1 M NaOH solution used was determined.
Other changes like the percipitate or the blue layer were because of concentration change. The observations made support the conclusion, as the colors did change due to the equilibrium shift. Although by observing the qualitative data we can see that the results observed may be inefficient because it was based only on our observasions and we could have different perspectives on the colors. To further this experiment you would look into other complex’s that could further affect the Cobalt Chloride. Looking into what other stress’s that could be added to shift the equilibrium constants.
The absorbance level @ 520 nm obtained from the spectrometer indicates the amount of urea obtained via measuring the absorbance of the light through the supernatant coloration, which was provided by the
