How The Rate Of That Ethanol Produces Ethanal By Potassium Dichromate

Ethyl ethanoate is made from ethanol and ethanoic acid. In the reaction sulphuric acid is added as a catalyst.

The method used in this experiment is called an oxidation reaction. An oxidizing agent takes away electrons from other reactants during a redox reaction. The oxidizing agent typically takes these electrons for itself, thus gaining electrons and being reduced (Helmstein, Ph. D 2017). The organic oxidant used in this experiment is sodium hypochlorite, which is also known as “household bleach’. Sodium hypochlorite in acetic acid is an alternate oxidizing agent used for the development of ketones that was developed by Stevens, Chapman and Weller due to the many advantages it displays (J. Org. Chem, 1980, 45, 2030). This particular oxidation of sodium hypochlorite is an exothermic reaction meaning that it releases heat as an energy form. Due to the exothermic nature of this experiment, temperature ranges should be monitored throughout the experiment. The overall objective in this experiment is to yield a

Abstract: Using hypochlorous acid to convert secondary alcohol called cyclododecanol to the corresponding ketone which is cyclododecanone by oxidation.

(0.074 mol HCl x 1 mol NaOH) / 1 mol HCl = 0.074 mol NaOH

In the Cannizaro reaction an aldehyde is simultaneously reduced into its primary alcohol form and also oxidized into it 's carboxylic acid form. The purpose of this experiment is to isolate, purify and identify compounds 1 and 2 which contain 4-chlorobenzaldehyde, methanol, and aqueous potassium hydroxide. Compounds 1 and 2 are purified by crystallization. . The purified product will be characterized by IR spectroscopy and melting point.

During the experiment, two different techniques to disturb systems at chemical equilibrium are utilized. The first one is changing the concentration of one of more species that are involved

KIO3 + 6 HCl + 6 Na2S2O3 → 3 Na2S4O6 + KI +3 H2o + 6 NaCl

(aq) + HCO3- (aq)  Ni(HCO3)2 (s) + 2 Na+ (aq) + 2 NO3- (aq)

We tested the different reactions of each chemical compound that we used with the flame. The purpose was to see the electron excitation of each reaction and the color that it emitted. Also, to see the color of each reaction determining the amount of energy released using our color scale.

In the hypothesis it was predicted that the Glucose (C12H12O6) would react with the water in the presence of a catalyst, which would speed up the rate of reaction. In this reaction Glucose would react with water to produce Carbon Dioxide (CO2) and Water (H2O). Methylene blue was an indicator that turned blue as it reacted with the Oxygen in the water. In a perfect case scenario, the dissolved oxygen in the water would cause the Methylene blue to turn blue. As the reaction takes place, the oxygen is consumed in the reaction as glucose is oxidized to form carbon dioxide and water thus, turning the solution colorless. As the flask is mixed, the oxygen is dissolved back into solution therefore converting the color from colorless

The experiment is carried out on paper where you put a spot of the chemical near the bottom of a chromatography piece of paper and the paper is in a solvent which is usually water. When the solvent (water) soaks up the paper it carries the chemical up with it. Different components of mixtures will move at a different rate as other, some would move faster or slower than others which separates the mixtures from each other. Paper chromatography works because some of the colours are better at dissolving in liquid than they are bonding with the paper so that means they will travel further up the chromatography

Being that the indigo dye is made up of several complex compounds, the product of the reaction and reacting ratios may be difficult to determine; however, the stoichiometric ratios as well as the substances produced do not need to be known to calculate the rate; as the disappearance in colour is being measured by a colorimeter.

where ci is the molar concentration of species i (mol L−1 ; usually denoted by species in brackets) and ρ is the density of the solution (kg L−1 ). Inserting Eq. (17) into Eq. (16) we have: H3 O+ A− ρbθ [HA]

1. When hexane was initially added to the separatory funnel with the acetone the result was that the solution became very dark green at the top. There was a gradual color increase in the intensity from the bottom of the funnel to the top from a lighter green to a very deep dark green at the top.

(NH 2 ) 2 CO + 3H 2 O ----------> 2NH 3 (aq) + CO 2 (g)