Lab Report On The Equation

The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions.

The experiments conducted for this lab report focused on water contamination and filtration. Experiment 1 was effects of groundwater contamination. Oil, vinegar, and laundry detergent were added to clean water with no means of filtration. The clean water was found to be contaminated. A filtration system consisting of cheesecloth and 60 ml of soil was created and the contaminated samples were filtered through it. The soil and cheese cloth did not affectively filter the contaminants. Experiment 2 focused on

The Oxidation of a Secondary Alcohol with Sodium Hypochlorite experiment was performed to show how to change an unknown alcohol into a ketone. The unknown that was found for this experiment was Compound A. Once the ketone was found from the unknown alcohol, an IR and the boiling point was taken to try and figure out what the product and starting alcohol actually is. The first thing that is added to the 1.50 g of unknown compound A is 15 mL of 8.25% of NaOCl, which is a bleach solution. This reacted with the alcohol so the solution could then be tested using the iodide-starch paper. The reaction came out positive when tested because a blue, black spot appeared on the strip.

Approximately 0.05 g of 9-fluorenol, 250mg of chromic oxide resin, and 2 mL of toluene were used for the reaction solution. The CrO3 resin consisted of little brown solid balls. The reaction solution was slowly heated to 130°C. The reaction solution slowly turned light yellow as it was being heated. 1M standards for 9-fluorenol and 9-fluorenone were used. The reaction mixture had a strong gas-like odor while it was filtered through the Hirsch funnel. After evaporating the solvent using a rotary evaporator, the crude product that was left was yellow and solid. When hexane was added the yellow solid formed into a yellow liquid.

ssion In this experiment, 2-ethyl-1,3-hexanediol was reacted with sodium hypochlorite in an attempt to identify how sodium hypochlorite acts as a reagent. Due to the nature of 2-ethyl-1,3-hexanediol we are able to determine if sodium hypochlorite is a selective reagent. 2-ethyl-1,3-hexanediol has 2 alcohol functional groups with one being primary and the other being secondary. A selective reagent is one which oxidizes one functional group although its in the presence of 2 or more.

Discussion: The main scientific concept explored in this laboratory was the ability to observe the chemical reaction between Fe and Cu and to determine the ratio of moles of iron used to moles of copper produced in the reaction. A chemical reaction occurred when we used 4.06 grams of copper (II) chloride and mixed it with 9.43 grams of iron nails. The copper (II) chloride used 1.24 grams of iron from the nails to produce 1.99 grams of copper solid.

After completing my experiment I came to a number of conclusions for each solute, the first solute that I tested was Potassium chloride and as soon as I finished recording my data I came to a number of interesting conclusions. First, as mentioned in my observations, in each attempt the numbers were very similar in conductivity. This means that the data collected was very accurate since the numbers didn't change to much. Also, the Potassium chloride was the hardest solute to dissolve in water. This means that the solute is very saturated comparing to the other solutes that I tested. In conclusion the Potassium chloride was very unique comparing to the other solutes that I tested throughout my experiment.

The purpose of the experiment is to oxidize a secondary alcohol (2-octanol) by using sodium hypochlorite (bleach) to produce 2-octanone. The starting material consisted of a sample of 2-octanol that was placed into a three-neck flask along with acetic acid and acetone creating an acidic solution. While monitoring temperature fluctuations to ensure a temperature of 400 Celsius was not reached, sodium hypochlorite slowly dripped from a separatory funnel into the acidic solution. Once this reaction reached its entirety, the solution was combined with sodium bisulfate to remove any of the remaining oxidizing agent. This solution was then tested and brought to a neutral pH using a sodium hydroxide solution. The reaction material was extracted using ether and was then washed with a saturated sodium chloride solution. The organic solution was then dried using magnesium sulfate and was then decanted and placed onto the rotovap. The produced weighed .599g and based on the infrared spectrum analysis (see Figure 1) preformed on the product it was determined to be 86.1% 2-octanol, which means .516g of 2-octanol was obtained in the final product.

3. A few drops of 6 M acetic acid were added until it became basic.

Chemical Equilibrium Ben Cooper TA Kia Williams CHM2046l.004 20 April 2015   Introduction Chemical equilibrium is defined as “a state in which the rate of the forward reaction equals the rate of the backward reaction” [1]. Equilibrium constant, defined as “a number that expresses the relationship between the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature” [2]. The equilibrium constant, Keq, was found by multiplying the products’ concentrations, then dividing it by the equilibrium concentrations product of the reactant. Small Keq values means that the reaction does not fully go to completion. When looking at a large Keq value, the reaction entirely goes to completion therefore

The overall goal in this lab was to oxidize borneol, a secondary alcohol, into camphor, which is a ketone. For the purposes of oxidation chromic acid was utilized, which was prepared by adding a 1:1 ratio of chromium trioxide to dilute sulfuric acid.

In this experiment, a redox reaction occurred. An oxidation-reduction reaction (redox) is a type of chemical reaction that involves a transfer of electrons between two solutions. The chemical being oxidized is losing electrons and the chemical being reduced is gaining electrons. In this case KMnO4 is losing electrons and Oxalic Acid is gaining electrons. KMnO4 can titrate a or reduce Oxalic acid. Titration is the technique used to find the unknown concentration of one solution based on the concentration of a known solution. In equation 2, the molar relationship between the 2 is shown, it is 2 KMnO4 to 5 Oxalic Acid. The molar ratio relationship is useful because it shows how much of a certain product is needed to help a reaction occur and which chemical is limiting reagent. The experiment was started by preparing a titrating strength KMnO4 solution from stock to a less concentrated KMnO4. Equation one shows how this was done. The KMnO4 needed to be diluted, if it had not been diluted, then it would be way too hard to get an accurate reading of the Oxalic Acid used. Without being diluted the Oxalic Acid would be strong. The next step was to standardize the KMnO4 solution. It was calculated that 37.5 mL of Oxalic Acid could titrate 15 mL of KMnO4. To determine the exact molarity of a solution a standardization needs to happen. In this experiment the standardization found how much Oxalic acid was needed. Through the controlled variable, the fact that 37.5 Oxalic acid could be titrated by 15 mL of KMnO4, the percent of the

Chemical equilibrium is the study of change within a chemical reaction and how far it will go to reach a dynamic equilibrium (Burdge). Dynamic equilibrium is defined as the constant movement of species in a chemical reaction, gone to incompletion while the rates of production and consumption are equal (Kf = Kr ) (Burdge). It differs from static equilibrium in that species are constantly being consumed and produced, it is dynamic movement (Fox). The concentration of such species do not change, it remains constant (Fox). The rate at which species are being consumed and produced is known as the equilibrium constant (K) (Burdge). Due to the fact that the concentration

Subsequently, 10mL of 3.5% H2O2 were added dropwise to the reaction mixture and was stirred for 20 minutes before heating to boiling at 80°C for 5 minutes. The reaction mixture was then taken off heat and allowed to cool undisturbed in an ice-bath for 30 minutes. Suction filtration was performed after to collect the crystals from the chilled solution The product was then washed with chilled 95% ethanol (2 x 15mL) and followed by diethyl ether (2 x 10mL). The crude product was then left to dry before recording the yield. 20mg of the crude product is then accurately weighed out and dissolved in deionized water in a 25mL volumetric flask. Deionized water was added to the volumetric flask to the mark and the UV-vis absorption spectrum of the crude product was recorded.