which the acceptance of an electron (reduction) by a material is matched with the donation of an electron (oxidation). A large number of the reactions already mentioned in the Reactions chapter are redox reactions. Synthesis reactions are also redox reactions if there is an exchange of electrons to make an ionic bond. If chlorine gas is added to sodium metal to make sodium chloride‚ the sodium has donated an electron and the chlorine has accepted an electron to become a chloride ion or an attached
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Exercise 7.3 (training!!!) 1. Find the oxidation numbers of the underlined elements in the following species. (a) (e) (i) (m) (q) (u) (y) 2. SO3 PbSO4 CoCl42CrO42SO32Ca(NO3)2 Co(NH3)43+ VO2+ CaH2 KMnO4 SCl2 N2 NaOH (c) (g) (k) (o) (s) (w) HCO3[Al(OH)4]MnO42NO2FeCl3 KOCl (d) (h) (l) (p) (t) (x) H2S2O7 H2O2 Cr2O72K2SO4 CH4 Pt(CO)4 Which of the following equations represent redox reactions? Specify the species being reduced in each case if applicable. (a) (b) (c) (d) NaI(s) + 2K(s) + 2NH3(g)
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Green Oxidation of Borneol to Camphor Abstract: This lab converted borneol to camphor using a green oxidation. Sodium hypochlorite was used instead of the less “green” Jones reagent. Borneol was mixed with glacial acetic acid and oxidized with sodium hypochlorite to make crude camphor. The crude camphor was purified by sublimation. The final product was characterized by obtaining a melting point and inferred spectroscopy. The experiment was carried out to see if bleach could oxidize borneol
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OXIDATION-REDUCTION TITRATIONS REDOX TITRATION • involves oxidizing agents and reducing agents titrants and analytes • oxidizing agents used as standard solutions: potassium permanganate‚ KMnO4 potassium dichromate‚ K2Cr2O7 iodine‚ I2 ceric sulfate‚ Ce(SO4) 2 potassium iodate‚ KIO3 REDOX TITRATION • reducing agents used as standard solutions: ferrous sulfate‚ FeSO4 oxalic acid‚ H2C2O4 sodium oxalate‚ Na2C2O4 sodium thiosulfate‚ Na2S2O3 titanous chloride
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EXPERIMENT 3 DETERMINATION OF ORGANIC MATTER BY WALKEY- BLACK WET OXIDATION METHOD OBJECTIVE: This method determines the percentage of organic carbon and organic matter in the soil. INTRODUCTION The soil sample is suspended in standard potassium dichromate (K2Cr2O7) solution to which concentrated sulphuric acid is then added. The heat generated on adding the sulphuric acid and the presence of chromic acid creates strong oxidizing conditions. The excess chromic
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Precipitation of Sulphur 2HCl(aq) + Na2S2O3(aq) ⎯→ 2NaCl(aq) + S(s) + SO2(g) + H2O(l) Na2S2O3: Sodium thiosulphate Notes: 1. Yellow precipitate (sulphur) is formed. 2. The reaction is slow. Potassium Dichromate (VI) with Ethanedioic Acid Cr2O72- + 14H+ + 3C2O42- ⎯→ 6CO2 + 7H2O + 2Cr3+ Notes: 1. In the reaction‚ the orange colour of the solution turns into green. Cr2O72-: dichromate(VI) ion (Orange) C2O42-: ethanedioate ion (Colourless) Cr3+ : Chromium(III) ion (green) Potassium
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alkali‚ allergic contact dermatitis‚ cement‚ chromate eczema‚ chrome‚ chromium‚ clinker‚ Cr (VI)‚ Cr (III)‚ ferrous sulfate‚ finish mill‚ health‚ hexavalent‚ kiln atmosphere‚ manganese sulfate‚ Occupational Safety & Health Administration‚ OSHA‚ oxidation‚ portland cement‚ raw materials‚ reducing agent‚ refractory brick‚ solubility‚ stability‚ stannous chloride‚ stannous sulfate‚ storage period‚ trivalent. ABSTRACT With regard to chromium and health and safety aspects‚ the water-soluble compounds
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Experiment # 1 Date: 18/12/13 Title: Chemical Properties of Alkanes. Aim: To test the reactivity of alkanes using cyclohexane as an example. Apparatus/Materials: Cyclohexane‚ liquid alkane‚ aqueous bromine‚ test tubes‚ light source‚ watch glass‚ splint‚ 0.1 MKMnO4‚ concentrated H2SO4‚ dilute H2SO4. Method: Combustion: 1. A watch glass was placed on a benched protection sheet in a fume cupboard and the extractor in the fume on. 2. 4 drops of cyclohexane was placed on the watch glass using
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2011 Objective: The purpose of this experiment was to synthesize adipic acid from cyclohexanol via an oxidation reaction that was catalyzed by sulfuric acid. Purity of the product was assessed by measuring the melting point. Physical Properties/Structures: Name | Formula | Molecular Weight (g/mol) | Boiling Point (0C) | Melting Point(0C) | Density(g/mL) | Hazards | Sodium Dichromate Dihydrate | Na2Cr2O7 . 2H2O | 297.98 | 400.0 | 357.0 | 2.35 | -Eye/skin irritant-Affects Respiratory System
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Q.1 Bond enthalpy of fluorine is lower than that of chlorine‚ why? Q.2 Give the IUPAC name of the following compound: (CH3)3-C-C-COOH ║ O Q.3 On increasing temperature‚ activation energy of a reaction decreases‚ why? Q 4 Which of the following is most effective electrolyte in the coagulative of AgI/Ag+sol? K2SO4‚ MgCl2‚ K4[Fe(CN)6] Q.5 Write the reaction when glucose is heated with excess of HI. Q.6 Which Xe compound has distorted octahedral shape? Q.7 What is the denticity of
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