2. Qualitative ORGANIC functional group tests in various homologous series | TEST FOR | TEST METHOD | OBSERVATIONS | TEST CHEMISTRY and comments | ALKENE or alkyne i.e. any non-aromatic unsaturated hydrocarbon with a double or triple carbon-carbon bond. | Bubble gas through‚ or add liquid to‚ a solution of bromine in hexane or water. | The orange/brown bromine rapidly decolourises‚ as a saturated colourless organic bromo-compound is formed. | R2C=CR2 + Br2 ==> BrR2C-CR2BrRCCR + 2Br2 ==> Br2RC-CRBr2R
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reactions below‚ (i) state and explain what would be observed; and (ii) write an appropriate equation. (a) adding excess sodium sulphite solution to iodine solution (b) adding aqueous chlorine to potassium bromide solution (c) adding excess potassium iodide solution to acidified potassium permanganate solution 1 (d) adding excess iron(II) sulphate solution to acidified potassium dichromate solution (e) adding concentrated nitric acid to magnesium ribbons (f) (g) (h) (i) (j) (k) (l) (m) (n) 5. adding
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Links: Jump up ^ Nyholm‚ R. S.; Woolliams‚ P. R. (1968). "Manganates(VI)". Inorg. Synth. Inorganic Syntheses 11: 56–61. doi:10.1002/9780470132425.ch11. ISBN 978-0-470-13242-5.
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The reaction of Hydrogen Peroxide and Iodide ions in an acidic medium: 3 I-(aq) + H2O2(aq) + 2 H+(aq) I3-(aq) + 2 H2O(l) Step 1. H2O2(aq) + I-(aq) IO-(aq) + H2O(l) Step 2. IO-(aq) + H+(aq) HOI(aq) Step 3. HOI(aq) + 2 I-(aq) + H+(aq) I3-(aq) + H2O(l) In this reaction the three iodide ions are oxidised to form the triiodide ion. This occurs in three steps. Firstly‚ the peroxide molecule oxidises a single iodide ion‚ to form a hypoiodite ion‚ and a molecule of water. This is the
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sulphate ions are present. The chemical equation for this reaction is: Fe2(SO4)3(aq) + BaCl2(aq) FeCl3(s) +
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+ I2 Br2 + 2I- ( 2Br- + I2 • Down the group the outer electron is further from nucleus and more shielded so gained less easily 3) Trends in properties of the halides • The halides (chlorides‚ bromides and iodides) are reducing agents which lose an electron when they react • The ability to act as a reducing agent increases down the Group • Down the group the outer electron is further from nucleus and
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Filiz‚ N.A. Sayar and A.A. Sayar‚ Hydrometallurgy‚ 2006‚ 81‚ 167–173. 6. ^ Yoshinari Baba‚ Minako Iwakuma and Hideto Nagami‚ Ind. Eng. Chem. Res‚ 2002‚ 41‚ 5835–5841. 7. ^ J. M. Sánchez‚ M. Hidalgo‚ M. Valiente and V. Salvadó‚ Solvent Extraction and Ion Exchange‚ 1999‚ 17‚ 455–474. 10. ^ P. Giridhar‚ K.A. Venkatesan‚ T.G. Srinivasan and P.R. Vasudeva Rao‚ Hydrometallurgy‚ 2006‚ 81‚ 30–39. 11. ^ K. Takeshita‚ K. Watanabe‚ Y. Nakano‚ M. Watanabe (2003). "Solvent extraction separation of Cd(II) and
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reaction has many alterations‚ the alteration used in this investigation is hydrogen peroxide and includes the use of‚ sodium thiosulfate‚ potassium iodide‚ and hydrogen peroxide. The use of starch solution is essential in this experiment as it acts as an indicator for the experiment turning the color of the solution dark blue in the appearance of iodine ions. This allows the end of the reaction to be determined. The clock reaction is shaped by two different reactions. The first reaction is the slow
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CHEM 1112 Kinetics of the Persulfate – iodide Clock Reaction The purpose of this experiment is to determine the rate law and the activation energy for the reaction between persulfate ion‚ S2O82-‚ and iodide ion‚ I-: S2O82-(aq) + 2 I-(aq) 2 SO42-(aq) + I2(aq) The rate law can be written as Reaction rate = (1) Where m and n are the orders with respect to S2O82- and I-‚ respectively‚ and k is the rate constant. Determining the rate law involves determining the values
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Chemistry Lab Report (Design) Factors affecting Rates of a Reaction (Kinetics) KINETICS DESIGN LAB Research Question: Does the concentration of Potassium Iodide (KI) affect the rate of its reaction with hydrogen peroxide (H2O2) (of a fixed concentration)? Introduction: There are several factors that affect the rate of a reaction. Some of them being Pressure (if the reactants are Gases)‚ Temperature‚ Presence of a Catalyst‚ Surface Area of the reactant‚ and Concentration. According to
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