Electric Hot Plate Lab Report

The purpose of this lab was to determine the empirical formula of copper oxide compound. In the lab, hydrochloric acid and copper oxide compound was mixed until it formed a blue solution. An oxidation-reduction reaction, a reaction in which there is an exchange of electrons between elements, was performed by adding zinc to the solution to displace the copper in copper chloride. Zinc, in this case, was oxidized by losing two electrons (0 → 2+) while copper was reduced by gaining two electrons (2+ → 0). Also, when the copper was displaced, it became a precipitate, which is a substance that comes out of a solution as a solid due to insolubility.

After this, the solution was poured into a volumetric flask just about to the 1dm3 line and then it was left there to cool to the same temperature as the room before filling precisely to the 1dm3 line with distilled water. The molar mass of CuSO4.5H20 was 249.5 so that means 249.5g of copper sulphate was needed to dissolve, in order to make a standard solution, into 1dm3of distilled water. Following this, a linear dilution of the CuSO4.5H2O was made in order to be used to make a calibration curve after using the colorimeter to write down the absorbance of each sample. A linear dilution is diluted with distilled water in order for it to make the concentration weaker and weaker. For this investigation, the dilutions made ranged from 0.01 to 0.1 M/l . It was essential to only make up 10cm3

In this experiment an elemental copper was cycled a series of five reactions where it ended with pure elemental copper as well, but at different stages of the cycle the copper was in different forms. In the first reaction, elemental copper was reacted with concentrated nitric acid where copper changed the form from solid to aqueous. Second reaction then converted the aqueous Cu2+ into the solid copper II hydroxide (Cu(OH)2) through reaction with sodium hydroxide. The third reaction takes advantage of the fact that Cu(OH)2 is thermally unstable. When heated, Cu(OH)2 decomposes (breaks down into smaller substances) into copper II oxide and water. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion (Cu2+). The cycle of reactions is completed with the

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

The purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

The purpose of this lab is to determine the percent of water in a hydrate. I learned that copper sulfate hydrate is blue on its own but, when heat is added it will change color to a dim gray. One error that may have occurred is the failure to zero the scale which would ultimately change the math in the equation. Another error that may occur in this lab is forgetting to wait the recommended amount of cooling time, which would change the mass of the elements. At the end if the lab when we look to the questions, it is also beneficial to look at the notes for the lab because it helps with the setup of equations that may come with the questions, also it is very helpful

The main purpose of the lab “Determination of the Formula of a Copper Oxide” was to determine the formula of a copper oxide. Specifically, this is a compound of copper combined with oxygen. This was to be done by heating the copper oxide thoroughly until all of the oxygen had been driven off. To accomplish this experiment, we first had to take and measure the mass of a specified color of copper oxide, ours being red. Then, we used a fischer burner to provide the heat needed for the split of copper oxide, in which our amount resided in a test tube. But, in order for the copper to not recombine with oxygen that could be found in the surrounding atmosphere of our lab, we also had to have a flow of methane gas into the test tube that fed into

In this experiment, the solid copper metal was weighed to get the initial mass to later compare the mass to the copper after all the reactions. The copper was put into a 250 ml beaker under the fume hood in order to measure excess amounts of 15.8 M nitric acid, HNO3 because the copper has to be the limiting reactant in order to change the state of matter of the copper. It needs to be aqueous instead of a solid. (Cu(s) + 4 HNO3 (aq) -> Cu(NO3)2 (aq) + 2 NO2 (g) + 2 H2O (aq)). After the reactants have reacted, 25 mL of water was added to the beaker to dilute the dangerous acid in the beaker for safety. Then 4 squirts of potassium hydroxide, KOH, was added to react with what’s now in the beaker, Cu(NO3), and this caused another reaction to happen (Cu(NO3)2 (aq) + 2 KOH (aq) -> Cu(OH)2 (s) + 2 KOH3 (aq)). Now the

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

In science I was forced to make a contraption that had to hold the heat in 200 milliliters of boiling hot water for as long as possible. We got two trials. One, to create an idea of what worked well, and what could be better. Two, to build off of our first trial and hopefully get a better result. From here we built our second and more efficient contraptions.

There are other systematic errors. For example, using inaccurate equipment which is scale. If the scale was not accurate, the mass of salt and sugar which were used in the lab would not be accurate. And the mass will affect the melting point time change. There are also some random errors.

The error may cause the amount of energy released to change due to different substances mixing up in the solution. This could have also been easily prevented by rinsing it with water or wiping it with a napkin every single trial. An important and common source of error would have been the substances reacting with water in the laboratory air since the substances were anhydrous or reacted with water. This could have occurred while the substances were being measured or grinded and it could have caused the amount of energy released to decrease due to the substance already reacting with the water in the air when it was added to the water in the coffee cup.

Energy is used in any type of reaction that causes a substance to change its phase. When heating a solid, energy is put into the substance, causing the substance to gain energy. If heating continues on the solid, a phase transition will occur and the solid will melt to a liquid. The amount of heat required to melt a solid to a liquid is an enthalpy, and is called heat of fusion. If the heating continues on the liquid, the substance will then reach its boiling point, and a phase change will occur again from a liquid to a gas.

Solutions of CuSO45H2O (0.506 g in 10mL water, 3.17E-3 mol) and ammonium peroxodisulfate (1.030 g in 10mL water, 4.51E-3 mol) were prepared and mixed

To determine the enthalpy change for the displacement reaction between zinc powder and copper (II) sulphate solution.