Sulfuric acid

Ever since the Industrial Revolution in the 18th century, fossil fuels have seen a huge rise in popularity. Used to power the economy and numerous factories, fossil fuels started the leap in technology that gives us the power we take for granted today. Since the beginning of the oil industry in the 19th century, petroleum has risen to global everyday usage. Initially kerosene, a product derived from petroleum, was used for lighting and heating, but with the appearance of oil drilling technology petroleum

many of the pieces have broken down. The beaker was rinsed with 10 mL of distilled water after the mixture was poured through the Büchner funnel of the aspirator. The filtrate was put into a clean 250 mL beaker to be added with 20.5 mL of 6.0M sulfuric acid, stirred slowly when added. The reaction was then put into a 1L beaker ¾ full of ice and water to kick start the reaction into making the alum crystals. The stirring rod was used to help activate the crystals. Once the making of the crystals had

compound by an electrophile. The rate and direction of the EAS reaction depends on the functional groups present on the aromatic compound. The purpose of this experiment was to synthesize bromonitrobenzene by reacting bromobenzene with sulfuric acid and nitric acid via EAS. Gas chromatography (GC) was performed on the product in order to confirm its identity by comparing its observed retention time to the true retention time of bromonitrobenzene. Additionally, the relative rates of reaction for several

Determination of the Composition of Cobalt Oxalate Hydrate Experiment 12 Robbie Kinsey Partner: Debnil Chowdhury Chem. 1312-D TA’s: Russell Dondero & Sylvester Mosley February 9, 2000 Purpose The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O. Procedure The powdered cobalt oxalate

The purpose of the experiment was to synthesize alum from aluminum foil, using a series of chemical reactions. The synthesis was achieved using sulfuric acid, potassium hydroxide, water, and aluminum. The synthesized alum was then used in a number of tests to test for the presence of ions in the compound (potassium, aluminum, sulfate, and water). The left over alum was then used to employ various techniques for crystal growth. In part one of the experiment, 0.251 grams of aluminum foil were obtained

100 mg each. It will then be dissolved in 1mL of each individual solvent such as distilled water, ethyl alcohol, chloroform, 1M Hydrochloric acid, 1M Sodium Hydroxide, and Diethyl ether. 1.5 Chemical Tests The chemical tests that will be performed would be fucose test to determine the fucose content, uronic acid test to determine the presence of uronic acid, sulfate ion tests to determine the presence of sulfate, carbohydrate tests to determine presence of carbohydrates and reducing sugars and, protein

The preparation of Grignard reagents typically involves the reaction of an alkyl halide or aryl halide with magnesium metal in an anhydrous ethereal solvent. This reaction results in the formation of a carbon-magnesium complex within an alkyl magnesium halide or aryl magnesium halide. Grignard reagents are considered to be strong nucleophiles and strong bases that have the ability to react with acidic proton sources and carbonyl functional groups. The preparation of Grignard reagents must be conducted

the benzene ring, which occurs because of ortho-para directing of activating groups2. Initially, to start this reaction, 6.5 grams of solid acetanilide must be placed into 10 mL of glacial acetic acid and fully dissolved over a steam bath then cooled via ice bath with 10 mL of concentrated sulfuric acid. After the mixture had cooled, a cold HNO3/H2SO4 solution was added slowly to ensure that the reaction would not occur to quickly, which would hinder the reaction process. The yellow precipitate of

oxide with the sulfuric acid electrolyte produces a voltage. The supplying of energy to and external resistance the battery. When a lead acid battery cell produces energy, it converts chemical energy into electrical energy. During this process, Lead is oxidised at the anode according to this equation: Pb(s) → Pb2+(aq) + 2e- The reduction process in lead acid batteries occurs at the cathode, as shown above. Lead (from lead dioxide) is reduced at the cathode by protons in the sulphuric acid: PbO2(s) +

resins and the extraction of the element will be conducted by using Zirconium from ores. Some of the resins used consisted of rare earths, beryllium, titanium and iron. John A. Ayers took zirconium ore’s and broke them down by using concentrated sulfuric acid. 8 Once the zirconium ore was broken down, the soluble zirconium was then converted to its nitrate form, Zr(NO3)4. The zirconium nitrate is then passed through a column containing a resin. The hydrogen form of Amberlite I.R.-100 was used as the