Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
4. Pour the salt-water solution into the water bottle. 5. Stretch the open end of the balloon around the mouth of the bottle and hold it there. 6.
After I rinsed the copper I transferred it to a watch glass that had been baked for 20 minutes so it would not contain any liquid so as to not counteract the experiment. After I put the copper on this watch glass I baked the copper in the oven for 20 minutes so there would be no liquid left in that to mess up the mass. After 20 minutes I removed the watch glass with the copper in it and weighed itm making sure to weigh the watch glass
The goal of this experiment is to find out what is the identity of the unknown hydrate? To answer this question first, we should know what a hydrate, and how to identify a hydrate using the law of constant proportions. A hydrate is a pure substance because it contains water molecules embedded in its crystal structure that does not vary. By heating the unknown hydrate, we can calculate the mass of the hydrated, and the percentage of water in the hydrate.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
The first experiment was a Synthesis reaction, this was done by burning the substance magnesium; the substances reacted to form one compound, which ended up being heavier than the first original mass of the magnesium, the final product was known as magnesium oxide. The second experiment that was conducted was the Decomposition reaction, which actually eliminated chemical elements by burning them off, therefore reducing the weight of the final product by 1.673 grams. The third experiment was known as single displacement, by adding the chemical hydrochloric acid to zinc it created a chemical reaction which actually increased the temperature, as well as the pressure within the flask. The last experiment that was conducted was known as double displacement, this experiment involved the exchange of bonds, between the two sodium hydroxide and nickel. The Nickel was forced to group together when it was placed into the sodium hydroxide, instead of mixing with the compound it would rather keep to
Then the flask was filled the rest of the way with distilled water to the mark. Similar steps were taken for the rock solution. The rock solution from the prior lab was filtered into a volumetric flask (100mL), then 15 M NH4¬OH (8mL) was added to the flask. After that, the flask was filled to the mark with distilled water. Both flasks were then swirled to combine the solution
Measure out 0.035 - 0.045g of magnesium ribbon and tie a string to it and record the mass of the ribbon. Pour 6 mL of HCl into the eudiometer. Carefully pour 50-60 mL of distilled water to fill up the rest of the eudiometer.
Gather materials (beaker, 100 milliliters of copper chloride, graduated cylinder, funnel, 2 centimeter by 15 centimeter aluminum foil strip, goggles, gloves, apron, hydrochloric acid, and a spoon to push down the aluminum foil so that it doesn’t rise up and drip copper chloride down the side) 2. Pour 100 milliliters of copper chloride into the graduated cylinder to measure it 3. Pour the copper chloride into the beaker or leave it in the graduated cylinder (whichever you want to conduct the experiment in) 4. Fold the tin foil in half the long way so that you have 1 centimeter by 15 centimeter strip of aluminum foil 5. Curl it into a coil/spring 6.
The Diels-Alder reaction, an electrocyclic reaction between a conjugated diene and a substituted alkene, also known as a dienophile, was used in the experiment. The purpose was to synthesize a substituted cyclohexene derivate by the reaction between the diene and dienophile, and it reacted in a reflux solution with toluene as the solvent forming an unsaturated six-membered ring. First, approximately 54 mg each of both compounds, tetraphenylcyclopentadienone (TPCPD) and diphenylacetylene (DPA), were placed in a reaction tube to be mixed and heated on a sand bath for several minutes. During the heating process, the color of the TPCPD reactant would fade as the color went from purple to white showing the other reactant. Also during the heating, DPA refluxed for a brief time until the tube was removed from the sand bath for the melted product to cool and solidify.
The purpose of this lab was to carry out two Diels-Alder reactions; Part 1 focused on obtaining, and characterizing through IR spectroscopy and melting point range, a diastereomeric mixture of 7-oxobicyclo[2.2.1]hept-5-ene-2,3-dicarboxylic anhydride produced from furan and maleic anhydride, while the goal in Part 2 was to produce dihydroanthracene succinic anhydride from anthracene and maleic anhydride and characterize the product using its melting point range. Since more extensive experiments such as mass spectroscopy, 1H NMR, and/or 13C NMR were not carried out in either part, the product structures’ cannot be confidently ascertained. Nonetheless, it will be assumed that at least the predicted products were isolated. For Part 1, the product in the reaction mixture was a near-transparent solid mass of prismatic crystals, while the isolated crystals were long, needle-like, and translucent white. This observation agrees with the literature appearance of “crystalline and white.”
Richard Heck is a chemist known for his works on carbon-coupling through the use of the atoms of the metal palladium to catalyze the bonding of carbons. This method was known as the Heck reaction. He was awarded the Nobel Laureate Prize in Chemistry last 2010 for his works that lead to a new way of innovation and inspiration to both young and old chemists. Heck was inspired to study science and in particular, chemistry from his interest in planting orchids when he was a child. As a teenager, he was interested in the chemicals that compose fertilizers and the pigments and nutrients of plants that lead to his eventual pursuance of chemistry through college and eventually earning himself a PhD at UCLA.
Place the the beaker onto a hot plate that is on a low heat setting (about setting 3). Every 5 minutes for 20 minutes, measure the circumference of the balloon and record it in Data Table A. You can measure the circumference of the balloon by looping a piece of string around it then using a ruler to measure the string’s length. Record the data in the data
In the first trial, measure 1.00M of hydrochloric acid into the graduated cylinder. Then enter your first whole 3cm piece of the magnesium strip into the cylinder. As soon as it starts reacting start the stopwatch. You will know it has started because it will start to bubble.
This experiment has to be carried out carefully
