125ml Erlenmeyer Reaction Lab

First, all of the equipment was obtained and placed on the table. The necessary equipment was weighed using a top loader balance, which used grams as its unit of measurement. The test tube, which held the samples, was filled with water from a plastic squirt bottle. A piece of filter paper, which had been folded several times, was placed over a funnel over an Erlenmeyer flask to filter the mixture in the test tube. The test tube mixture was poured onto the filter paper.

Type of Reactions We did a lab on many reactions to find the products of the reactions. We conducted four group experiments and three class experiments, following very strict safety procedures given to us by our instructor. We used goggles and aprons which were required at all times. We could not sniff any gasses or walk into clouds of smoke unless we were instructed to.

: During each reaction, something happened. During reaction 1, after adding the nitric acid a red-brown gas was created. The copper first turned green after a few minutes turned into a blue solution. Reaction 2, When acid was added a blue precipitate formed. Reaction 3, when heated the solution turned into a black precipitate.

For this experiment we are looking to determine the equilibrium constant KC for this reaction, KC = [FeSCN2+]/([Fe3+]•[SCN-]. Using a spectrophotometer, we are going to determine the absorbance of FeSCN2+ with different concentration measurements.

Two chemical reactions occurred in our lab and I have evidence to prove why. To start, the main purposes of the lab were to make two chemical reactions (which are the two main ingredients in the antacid Maalox), to learn about why changes in solubility, state, appearance, pH, and energy indicate that the chemical reaction really happened, and to learn about balanced equations and classifying them. In Part 1, we combined alum and ammonia to make aluminum hydroxide, potassium ammonium sulfate, and ammonium sulfate. In Part 2, we combined epsom salt (magnesium sulfate) and ammonia to make ammonium sulfate and magnesium hydroxide. But the two main ingredients are aluminum hydroxide and magnesium hydroxide.

After about an hour of reaction time, the mixture was isolated via vacuum filtration and was then acidified with 6 M HCl during the work up step. The reaction mixture was initially basic because of the sodium bicarbonate added during the beginning of the reaction. This was confirmed by a litmus paper test, with the reaction mixture spot showing up green which correlates to a pH of 8. However, the incorporation of HCl into the reaction mixture greatly acidified the solution. The litmus paper was spotted with the resulting reaction mixture and appeared red, which suggests a pH of about 2.

This report discusses how varying the mole ratio of the reactants affects the amount of the product that is produced and the amount of the reactants that remain at the end of the chemical reaction. We know that you can’t simply add another atom of nitrogen and take an atom of hydrogen away from ammonia because it would change to another substance. We also know that in a chemical reaction atoms cannot be created or destroyed but can make a new substance. A guiding question was made so they can figure out how to solve/find out what is going on. The atomic theory is connected to this lab because that the atoms in the lab cannot be created of destroyed during a chemical reaction. Meaning that each side the of the equation must include the same number of each type of atom. The relationship between the amounts of any two compounds, in moles, that are involved in a chemical reaction. In this lab we are showing how different ratios of moles of sodium bicarbonate and acetic acid and how the different moles leave and percentage out of the product but still remains in the lab. How this lab works we will combine sodium bicarbonate and acetic acid and we are see the amount of CO2 leftover after the reaction happens. Knowing this.

The ‘PT’ are the only subsets. If |V(T)| is even and T-clause is false, the verdict is unavoidable conflict.

The Diel-Alder reaction is a concerted cycloaddition between a diene and a dienophile. The first people to investigate this were Otto Diels and Kurt Alder, they were able to reported large variety of the dienes which turned out to be useful and so the procedure was named after them. This method is an efficient way to build rings that are stereospecific. A Diel-Alder reaction involves cyclic rearrangement of bonding electrons and forming and breaking bond(s) simultaneously.

The experiment requires a burette; 5-mL pipette; 2-mL pipette; 1-mL pipette; fourteen 50-ml glass-stoppered bottles; 0.5 N sodium hydroxide; phenolphthalein, methyl acetate, concentrated HCl, glacial acetic acid, and absolute methanol.

Once a reaction has reached its chemical equilibrium it consists of a point where the rates of the forward and reverse direction of a reaction equal each other. Since at this point there is no movement that needs to take place the chemical process can be considered to be stabilized. When a reaction has reached equilibrium, the reactants become products and the products decompose into the reactants at the same rate (Gas-Phase, 2014). In other words, the forward reaction must occur at the same rate as the reverse reaction. This all can be associated with Le Chatelier’s principle, which indicates that if the equilibrium is disturbed by any condition it will modify itself towards the direction of the change until it is fully balanced. (Gas-Phase,

In this lab section we talked about how elements on a periodic table are organized by increasing atomic number and we focus on six metals which are called Lithium,sodium,potassium,rubidium,cesium and francium. In which we observed how each metals reacted inside the water. To add on this lab focused on electrons and valence electrons. In which we learned that in a period table left to right it decreases and from top to bottom it increases. Before doing the lab we watched a video based on the lab we did. Then we wrote the observation we saw in video which were:

12 test tubes, 2 tube racks, liver, measuring cylinder, 6 beakers, hydrogen peroxide solution, stopwatch and ruler were collected.

The purpose of this experiment was to initiate and explore three different polymer reactions. One was an addition polymer reaction which used a mixing of chemicals and a boiling process to produce polystyrene. There was also two condensation polymers created, one through mixing compounds and shaking which is Bakelite, and the other through the careful mixing of compounds and pulling on the the surface where nylon has been produced.

Chemical kinetics is based on the use of an experimental rate law to determine the mechanism of a reaction. The experimental rate law for the given experiment can be found through the experimental instantaneous initial rate and the concentrations of each of the reactants present. First, using the equation rate = k[A]n[B]m, a ratio can be created of the rate equation of trial 1 to that of trial 2. These two trials are chosen because the concentration of reactant A is the same for both trials, so it can be simplified to one in the ratio. Since k is a constant and thus the same in both trials, it can be simplified to one in the ratio as well. After exchanging variables for the experimental data and simplifying, the resulting equation is 0.5 = 0.5m,