Manganese Synthesis Lab Report

Solar energy is already efficient with the environment; however, in order to solve this problem, we need to improve its efficiency with energy. In order for solar energy to be considered energy efficient today, we have to make the proportion of kilowatt hours produced over cost needed for it less than the proportion of this to fossil fuels. For example, in order to produce 1 kilowatt-hour or 3.6 megajoules, we need 50 cents. However, for coal in order to produce 1 kilowatt-hour for coal, we only need about 3 cents. Over the years, we have been decreasing the price little by little to now 18-30 cents, but this still cannot compete with fossil fuels that are all less than 10 cents. In order to solve this problem, we would need to improve the amount of energy received from the solar cells. We could achieve this by finding alternative materials to use on the cells to expand the

This lab could have contained errors. The errors could have happened when performing the lab. Some of the possible errors in this lab are:

Strontium nitrate, the limiting reagent, was poured into the copper(II) sulphate solution, the excess reagent, rather than the other way around. This is a minor systemic error, because even if some of the strontium nitrate remained in its initial beaker, the beaker was thoroughly rinsed out multiple times. The error causes the final mass of the filter paper and precipitate to be slightly decreased, as not all of strontium nitrate reacts with the copper(II) sulfate. This can explain why the percent yield in 92.2%.

This experiment is based on the concept of performing SN2 reactions and analyzing how different factors affect said reactions. The factors in question for this experiment are steric hindrance, nucleophilicity, and nature of the leaving group. An SN2 reaction is a type of substitution reaction. A substitution reaction entails an alkyl having its leaving group (typically a halogen) replaced by a different atom. A nucleophilic substitution involves a nucleophile attacking a leaving group on a carbon atom. The nucleophile utilizes its lone pair of electrons to form a new bond with the carbon atom. There are two different types of substitution reactions. There are SN1 reactions (first order) and SN2 reactions (second order) (Weldegerima 2016). SN1 reactions are unimolecular and involve two separate steps. One of the two steps takes longer than the other and is called the rate limiting step. SN1 reactions tend to favor tertiary alkyl halides. SN2 reactions involve a strong nucleophile interacting with an electrophile carbon and making the leaving group detach from the

In this modern fast paced world that we live in, there are many issues that are looked over, energy is one of these. As a world, we are dependant on dwindling fossil fuel supplies and take for granted electricity, oil, and gas. There are four completely renewable sources of energy around us that should be used and developed, they are: wind, growing plants, flowing water, and the sun. These sources of energy are the ones we should be tapping, because they are reliable and renewable. Harnessing the suns energy is the most certain and ultimate energy source. Looking at a brief history and some facts about solar energy, a glimpse of the future can be seen, a future not dependant on

The mean voltage of the battery terminals while connected to the identification resistors is presented in Figure ‎4 12. These samples have been pulled out from the voltage sensor of the PEB panel. The voltage decreased as expected from 12.53 to 12.5 during first 20 seconds of connection to the

Lab Title: Synthesis, Decomposition, Single Displacement and Double Replacement Chemical Reactions Purpose: The objective of lab four was to use the website Late Nite Labs to determine types of chemical reactions. Combining and/or heating various compounds, observing the reactions and balancing equations for the chemicals involved, reveals the chemical reactions. Materials: A computer, Internet, calculator and access to Late Nite Labs.

The purpose of this lab report is to synthesize luminol and then test its chemiluminescent properties. 5-nitro-2,3-dihydrophtalazine-1,4-dione was reduced using sodium hydrosulfite in a solution of 3 M sodium hydroxide in water to form luminol. The product was then used to chemically generate light by reacting luminol with 3 M sodium hydroxide, hydrogen peroxide, and potassium ferricyanide. The reaction created a bright, blue light emission. From glow sticks to revealing remnants of blood samples in crime scene investigations, luminol, C8H7N3O2, has a wide variety of real world applications.

For the Synthesis of Alum lab my lab group and I took 1 gram of aluminum foil and broke it into small pieces. Next we added 25 mL of 3M KOH solution. Once the foil was dissolved we filtered the solution through a Buchner funnel with filter paper sealed inside with water. As the solution was filtering we applied a vacuum filtration to the Buchner funnel to expedite the filtering process. Once it was completely filtered my lab group poured the solution into a beaker and covered the beaker with parafilm. We then waited overnight to allow the crystals to form inside the beaker. Unfortunately, we did not produce any crystals overnight so we borrowed some from another group. Once we obtained the crystals we had to stir them in a beakers to make more form other than just the ones we received. After we rinsed the crystals with half ethanol and half water mixture. Once they were dry we determined the mass of the crystals with a balance.

Results and Discussion Synthesis of Compound 3. Scheme 1: Synthesis of Compound 3. To synthesize compound 3, an approach involving treating triptolide with dimethyl sulfide and benzoyl peroxide in acetonitirile was used (Scheme 1). This approach resulted in the formation of compound 4 with a 51% yield and in triptonide (5) with a 46% yield.

In the three experiments that we did we extracted dan from strawberries, E.coli, and wheat germ. In each of the experiments we had to open the nuclear envelope in some way with the strawberries we did this by freezing them so that the expanding water would break the nuclear envelope and allow the dan to be extracted. We also smashed them up to help facilitate in the breaking up of the cells. In the wheat germ we used a mortar and pestle to grind the wheat into a fine powder to release the dna.

In the lab Which Is Your Metal, we attempted to identify an unknown metal by determining its specific heat capacity. We began by choosing a sample of metal, finding its mass, and describing it. We found the temperature of our boiling water. Then, we calculated the volume and temperature of the water in our calorimeter before and after the experiment. Through these calculations, we determined that the heat transferred to the calorimeter water from the hot metal was 595.65J (6.0x10²J with proper significant figures). After finding the heat transferred, we were able to calculate the specific heat capacity and match it to the correct metal. Our specific heat capacity came to 0.26J/g°C, which was closest to the

I. INTRODUCTION Cyanide is a chemical compound containing cyano (─C≡N) groups, comprising carbon and nitrogen radicals, and can be found in various organic and inorganic compounds. Some inorganic cyanide compounds such as sodium cyanide (NaCN) and potassium cyanide (KCN) are groups of compounds having negatively charged polyatomic cyanide ions (CN-). This compound is a salt of a highly toxic hydrocyanic acid. Several types of organic cyanides are usually called nitriles, in which the CN group is covalently bonded to a carbon group, such as methyl (CH3) dimethyl cyanide (acetonitrile). Since nitrile compounds do not release free cyanide ions, they are generally less toxic, or in the case of insoluble polymers such as acrylic fibers, essentially

In this experiment, methyl benzoate was synthesized from benzoic acid and methanol with acid catalyze using Fisher Esterification. First benzoic acid and methanol were mixed in 100 mL round bottom flask. We cooled the mixture in ice and poured 3 mL of conc. H2SO4 and swirled to mix compounds. Then we refluxed the mixture for 1 hour. We let the solution cool and then decanted into a separatory funnel containing 50 mL of water and rinsed the round bottom flask with 35 mL of tert-butyl methyl ether and added that to a separatory funnel. We shook and vented thoroughly and drained the aqueous layer which contained a bulk of methanol and H2SO4. We washed the solution in the separatory funnel with 25 mL of water, followed by 25 mL of sat. sodium bicarbonate

In the fifth reaction, 2.29 g of zinc was added to the copper (II) sulfate solution under the fume hood. The balanced equation for this reaction is written as followed: