undergo oxidation to form carboxylic acids in two stages‚ it forms an aldehyde and then to the acid. In this experiment‚ we are used to prepare benzoic acid from benzene. Potassium permanganate is used this operation as an oxidizing reagent‚ it is used to oxidize the benzoic acid as well as acting as a catalyst for the reaction. Potassium permanganate (KMnO4) is a very strong oxidant which is able to react with many functional groups‚ such as secondary alcohols‚ 1‚2-diols‚ aldehydes‚ alkenes‚ oximes‚ sulfides
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Experiment 7: Percentage Composition of Kclo3- A Gas law Experiment Anna CunananProfessor Stewart Chemistry 400 T/TH 1:30 PM 18 March‚ 2014 Objectives: In this Experiment‚ we will be decomposing KClO3 into two different compounds‚ KCl and O2. We are given a known mixture that has MnO2 in it to act as a catalyst. When decomposing KClO3 it releases O2 gas‚ which we then collect into the Erlenmeyer flask. The gas then displaces the water into the beaker‚ which we can then calculate the water evolved
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substances to see if they formed a double replacement reaction. We also looked for precipitants that were formed from the mixing of the different substances. We used barium nitrate‚ potassium hydroxide‚ sodium sulfate‚ magnesium nitrate‚ aluminum sulfate‚ and iron (III) chloride in set one. In set two we used potassium chloride‚ sodium hydroxide‚ magnesium nitrate‚ barium chloride‚ sodium sulfate‚ and magnesium sulfate. For each set‚ we mixed two drops of one compound in five wells of a spot plate
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How does a catalyst in the form of a metal ion affect the rate of reaction in an iodide clock reaction with potassium peroxydisulphate ions? Background When peroxydisulfate ions (S2O82-) react with iodide ions (I-) in the presence of a starch indicator‚ they produce a dark blue solution. Reaction (1) S2O82- + 3I- I3- + 2 SO42- (peroxydisulfate ion) (iodide ion) (iodine ion) (sulfate ion) To determine the rate law for this reaction a series of changes
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emission spectrum that shows colors of different spectrums hydrogen for example shows 4 colors …etc Materials: 1- Benson burner 2- A wire loop ( wake sure it ’s clean ) 3- 4 filter papers 4- 4 Unknown test solid as directed by instructor (potassium ‚ sodium ‚ calcium ‚ barium / chloride ) 5- A beaker 6- diluted HCL ( to clean the wire loop with it ) 7- A spatula
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providing this information in an editable file which can be sent to an instructor. obseRvations The color of the flame is expected to be as follows: Metallic ion Flame color Sodium Na+ Yellow/Bright Orange Strontium Sr2+ Red Potassium K+ Light Purple Barium Ba2+ Green Copper Cu2+ Green Lithium Li+ Red Calcium Ca2+ Orange Unknown Red-Strontium Questions A. All chemical used in this test are binary compounds. What portion of the periodic table is responsible
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Emission Spectra & Flame Tests Intro The emission spectrum is used in modern chemistry to help further studies of wavelengths and the spectrum. When a metal in a compound reacts in a flame and produces a color‚ it helps to show the strongest color in the emission spectrum. The purpose of performing these operations on the flame was to see how different metals would react. Using a spectroscope‚ it is possible to observe the line emission spectrum produced by sunlight‚ artificial light‚ and
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Kinetics of a Reaction I. List of reagents & products 1. 1.0 M Copper(II) nitrate (Cu(NO3)2‚ 0.10 M Hydrochloric Acid (HCl)‚ 0.010 M Potassium Iodide (KI)‚ 0.040 M Potassium Bromate (KBrO3)‚ 0.0010 M Sodium Thiosulfate (N2S2O3)‚ 2% Starch solution‚ Water (H2O) II. Summary of Procedure. Part 1: Find the Volume of One Drop of Solution 2. Fill pipet with 3ml of distilled water 3. Mass a beaker and record 4. Put 5 drops of water into beaker and record
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this experiment you will determine the percentage of oxygen in potassium chlorate. You will calculate the theoretical value from the chemical formula and compare your experimental value to the theoretical value. Background: When potassium chlorate (KClO3) is heated‚ it undergoes chemical decomposition. Oxygen gas (O2) is given off and potassium chloride (KCl) remains as the residue. The equation for the decomposition of potassium chlorate is: 2 KClO3 (s) 2
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iodine (part 2). For part 1 of the experiment‚ this was done by titrating a solution of 50 cm3 of diluted 0.0225M persulphate and 250 cm3 of 0.4M potassium iodine against a 50 cm3 solution of 0.01 M solidum thiosulphate‚ using 3 ml of 2% starch as an indicator. For part 2‚ a solution of 25cm3 of iodine and persulphate‚ and 25 cm3 of 0.04M potassium chloride was titrated against the same amount of thiosulphate. Using the titre values Tt (ml)‚ time (s) and Tinf‚ graphs were plotted in order to
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