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Stoichiometry introduction
Limiting reagent experiment
Limiting reagent experiment
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More handpicked essays just for you.
Stoichiometry introduction
Limiting reagent experiment
Limiting reagent experiment
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Recommended: Stoichiometry introduction
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
With the data collected from this chemical reaction percentage yield of the precipitate can be calculated to determine the effects of impurities in the reactants on percentage yield. PRE-LAB QUESTIONS 1. What is the balanced chemical equation for the reaction in this investigation? 2. Which reactant is considered impure in this investigation?
The purpose of this experiment was to prepare an unknown Grignard reagent and then identify the product by molecular weight and melting point. An IR reading was taken to further identify and validate what product was formed. DISCUSSION AND CONCLUSION Organometallic compounds consist of a carbon that is attached to a metal. The carbon atoms are strongly nucleophilic because of a partial negative charge that they carry.
The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.
In beaker with the formed CuSO4 from Reaction 4, a piece of aluminum wire, which was bent into a circular shape, was placed in the beaker, and completely submerged in the solution. To this beaker a small stir bar was added along with 5 drops of 6 M HCl to start the reaction. This beaker was place onto the hot plate, covered with a watch glass, and the stir setting on the hot plate was turned on so that the stir bar moved the piece of aluminum wire around and hit it repeatedly. The wire began to have copper form on it and the stir bar hitting the wire would knock off the formed copper. Before the beginning of the next step the reaction had to be completed.
Using the Law of Definite Proportions, the mass of this product was used to determine the number of moles of copper and chlorine in the sample, which led to being able to determine the
Purpose: To recognize the evidence of a chemical change and to prove the law of conservation of mass by observing a series of chemical reactions involving copper. A specific quantity of copper will be transformed through a series of chemical reactions to form new substances and then recovered as solid copper. A percent yield will be calculated to determine the amount of copper recovered from the chemical reactions.
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%.
The purpose of this lab will be to identify the percent yield of copper in the unbalanced equation _Al(s) + _CuCl2(aq) → _Cu(s) + _AlCl3(aq). This will be determined by cutting a piece of aluminium 9cm by 9cm, recording its mass in grams, preparing a copper (II) chloride solution using the weight tray and electronic scale to measure 5.0g of CuC12 and adding it to 100 mL of distilled water. Then, a stirring rod will be used to dissolve the piece of aluminium into the CuCl2 solution until it is no longer visible. Additionally, the mixture will be filtered using a filter paper (which was previously weighted) on a funnel and weighted after it is fully filtered. Furthermore, the chemical equation will be balanced, stoichiometry will be used to find
The copper(II) metal complex was prepared by reacting copper(II) chloride and sodium saccharinate together by applying heat. The copper(II) chloride was originally a white solid and the sodium saccharinate was a blue solid. A centigram balance was used to weigh out a 1.01g sample of the sodium saccharinate and a 0.75g sample of the metal salt, copper(II) chloride. Each reactant was placed in separate 50-mL beakers and then dissolved using 10 to 20-mL of deionized water. Once dissolved the reactants were combined into a 250-mL beaker along with a clean stir bar.
Ideally, every mole of each reagent would be used up, and theoretical yield, we are assuming that every last mole of the reactants would
Discussion 1) A balanced chemical reaction: Zn + CuSO4 ZnSO4 + Cu A full ionic reaction: Zn0(s) + Cu2+(aq) + SO42-(aq) Zn2+(aq) + SO42-(aq)
This equation will provide for the ability to calculate the moles of both the given and desired substances, which can be divided to find the theoretical yield. An experiment will then take place: first, it is important to properly clean a working station and to wear goggles and a lab coat. A beaker can then be filled with 10 mL of of water before gathering 2 g of solid copper (II) sulfate pentahydrate, 2 mL of 6 molar hydrochloric acid, and approximately .25 g of aluminum foil as provided; a scale can be used to keep these measurements accurate. Using a stirring rod, stir the hydrochloric acid into the water before placing the solid copper (II) sulfate pentahydrate into the beaker of water. Let the hydrochloric acid and solid copper (II) sit in the water for two minutes as the next portion of the experiment is prepared.
In this experiment, the ions that go through gravimetric analysis are the copper and sulfate ions (Grossie and Underwood, 25). Elemental analysis involves determining the amount, which is usually a percent, of an element present in a compound (Blauch, 1). In this experiment, the element going through the elemental process hydrogen, in which the percent of the compound is attempted to be found (Grossie and Underwood, 25). In order to find the amount of copper, copper oxine needs to be formed. To find it, there is a reaction of hydrated copper sulfate and oxine, producing copper (II) oxine (Grossie and Underwood, 25).