filings to the third and compared the rates of evolution of hydrogen gas in each test tube. 2.1.2. We mixed 3mL of 0.02 M KMnO4 and 2mL of 3 M H2SO4 in a test tube and stirred using a glass rod. Next‚ we divided the solution into two. We added 2mL of 0.03 M Na2C2O4 solution to the first half and 2 ml of H2O2 to the second and compared the rates at which the violet color of KMnO4 in the two test tubes disappeared. 2.2. Concentration 2.2.1. We placed into three separate test tubes 3mL of 12 M‚ 6
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with potassium permanganate due to saturate bond .Thus‚will forming two layer will form which the solution does not mix.While on the other hand‚2-pentene will react with sulphuric acid to form penta-2‚3-diol.The purple color of KmnO4 will change to brown CH3CH=CHCH2CH3 + KMnO4 (cold) ---> CH3CH2(OH)CH2(OH)CH2CH3 For the experiment between alkane and alkene that react with sulphuric acid‚alkene which is 2-pentene have react and change to ethyl hydrogen sulphate.The alkane‚heptanes doesn’t react as
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DOWNLOADED FROM WWW.STUDIESTODAY.COM DOWNLOADED FROM WWW.STUDIESTODAY.COM d – AND f – BLOCK ELEMENTS Electronic Configuration of Transition Metal/Ions The d-block element is called transition metal if it has partly filled d-orbitals in the ground state as well as in its oxidised state. The general electronic configuration of transition metal is (n–1) d1–10ns1–2. Exceptions in electronic configuration are due to (a) very little engery difference between (n–1) d and ns orbitals and (b) extra stability
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Lab #24- Preparation 4-Methylcyclohexene Introduction: The goals in this lab were to have a reaction occur with 4-methylcyclohexanol and an acid catalyst to form our product of 4-methylcyclohexene via an E1 reaction. This reaction is accomplished by removing the –OH group on 4-methylcyclohexanol via dehydration and to have a double bond form via a loss of a hydrogen on a β-Carbon. Many techniques and skills were developed in this lab. Among them were dehydration‚ isolation‚ drying
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Repeat the procedures using 5% NaHCO3. 9.3 Oxidation Reactions 9.3.1 Reaction with KMnO4 1. Prepare 4 test tubes with 2 ml of water and add 1 ml of conc. H2SO4 to each. 2. Place 4 drops (0.1 g) of formic acid‚ acetic acid‚ benzoic acid‚ and oxalic acid‚ each into a different test tube. 3. If the acid does not dissolve‚ place it in 50。C to heat until totally dissolved. 4. Add 3 drops of 5% KMnO4 to each‚ then shake and observe the reactions. 9.3.2 Reaction with Tollen’s Reagent
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is titrated until the end point and the final reading is recorded. The second reading is recorded in the usual manner. The experiment is repeated to obtain concordant results. (Titre highest - Titre lowest ≤ 0.10mL) The concentration of the KMnO4 solution is calculated in molL-1. A full report is written for this experiment: Title‚ aim‚ procedure‚ data recorded‚ calculation and results‚ discussion (random error source and minimization explained; possible systematic error source identified
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exercise‚ we will determine the Percentage Oxalate Ion (C2O42-) in our Potassium Ferric Oxalate Trihydrate (K3[Fe(C2O4)3]•3H2O) sample using a technique called Titration; a type of Volumetric Analysis. This will involve adding a Potassium Permanganate (KMnO4) solution‚ whose concentration is previously determined‚ to a solution of the Oxalate until the reaction between these species is complete. By knowing the reaction stoichiometry‚ the volume Permanganate Ion (MnO4-) solution required‚ and the concentration
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carbocation more than just a normal secondary carbocation. 5. You ran 2 “qualitative” tests for unsaturation on your product. a. Describe what you observed when the Baeyer (KMnO4) test was run on your sample. After four drops of the product was placed in a small beaker along with ~0.5ml of acetone‚ three drops of KMnO4 was added. The mixture soon turned into a darkish brown color which concludes a positive for a Baeyer test. b. Describe what you observed when the Br2 in CH2Cl2 test was run
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Determination of Manganese in Steel Submitted by: ------------------- Date of Submission: 27.03.11 Objectives: In steel production aside the iron‚ which is the primary source‚ some amounts of manganese is used together with carbon. The objective of this experiment is determining the manganese amount in the steel compound by using UNICAM UV-VIS Spectrometer. Theory: Many molecules absorb ultraviolet or visible light. The absorbance of a solution increases
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Since the MnO4 ion is a deep pink-violet colour and the Mn2+ ion is nearly colourless‚ the end point in titrations using KMnO4 can be taken as the first pink colour that persists in the solution. In titration ‚ permanganate solution is put in the burette and is run down to an acidified solution of reducing agent‚ e.g..ammonium iron(II) sulphate solution.In this experiment‚ KMnO4 will be used to determine the percentage of Fe2+ in an unknown solid sample dissolved in water. The permanganate oxidation
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