ACKNOWLEDGEMENT The success of this investigatory project is directly related to the contributions of the ever supportive persons in my aura: To my friends who were there to cheer me up in time of doing this investigatory project‚ “Thank you so much!” To my parents who help me in providing significant material contributions‚ “Thank you and I love you so much!” To my adviser‚ Analiza R. Barcarse for her exquisite attention in guiding me‚ “Thank you‚ Ma’am!” To Ms. Estrella B. Acosta‚ the Science
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re-dox process – there is oxidation # changes with specific elements. Oxidation# increases = oxidation; Oxidation # decreases = reduction. Oxidation and reduction always happen within the same reaction. 2. Separate into 2 half-reactions. One show oxidation and the other reduction. 3. Balance the half equations for mass – only for the key elements at this time. 4. Balance the half equations for charge – adding e’s. * Find change of the oxidation number of a specific
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an oxidation- reduction reaction. • To determine the concentration of an unknown sodium oxalate (Na2C2O4) solution by titrating it against standardized potassium permanganate solution (KMnO4). • To determine the percent by mass of Fe(II) in the form of ferrous ammonium sulfate Fe(NH4)2(SO4)2.6H2O in a mixture by redox titration. B. Theory: (electron transfer reactions) 2Mg (s) + O2 (g) 2MgO (s) 2Mg 2Mg2+ + 4e- O2 + 4e- 2O2- Oxidation half-reaction
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Oxidative System • ATP yield: depends on substrate – 32 to 33 ATP/1 glucose – 100+ ATP/1 FFA • Duration: steady supply for hours • Most complex of three bioenergetic systems • Occurs in the mitochondria‚ not cytoplasm 4 Oxidation of Carbohydrate • Stage 1: Glycolysis • Stage 2: Krebs cycle • Stage 3: Electron transport chain Figure
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90696 906960 For Supervisor’s use only 3 Level 3 Chemistry‚ 2008 90696 Describe oxidation-reduction processes Credits: Three 9.30 am Friday 28 November 2008 Check that the National Student Number (NSN) on your admission slip is the same as the number at the top of this page. You should answer ALL the questions in this booklet. A periodic table is provided on the Resource Sheet L3–CHEMR. If you need more space for any answer‚ use the page(s) provided at the back of this booklet and clearly
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or polyatomic. The simplest compounds to name are binary ionic compounds‚ for example NaCl‚ which is named Sodium Chloride. Na having a positive oxidation number goes first followed by Cl which having a negative oxidation number goes last and is changed from Chlorine to chloride the -ide indicating its negative charge. Of course‚ the
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brass and bronze‚ are very important Has various oxidation states: 0 in elemental copper‚ +1‚ and +2 which is observable in corroded brass/bronze Oxidation states n n n Oxidation state is an indicator of the degree of oxidation of an atom The formal oxidation state is the theoretical charge the atom would have of all bonds were 100% ionic Oxidation is loss of electrons‚ reduction is gain of electrons (OIL RIG) Oxidation States of Copper n n n n n 0
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subsequent oxidation in solution to adipic acid using an excess of strong nitric acid. This report deals with KA oil/cyclohexanol production by various routes‚ followed by the common step of nitric acid oxidation. KA oil production from cyclohexane by the cobalt catalyst and boric acid air oxidation routes is reviewed. Production of KA oil from phenol is also covered‚ as is the Asahi process for cyclohexanol production from benzene via cyclohexene. Appropriately adjusted nitric acid oxidation is appended
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that all three alcohols should have a different level of reactivity. The hydrogen atom on the hydroxyl functional group can be easily substituted because of its enhanced acidity. This is the basis of a halogenation reaction‚ and controlled oxidation reaction‚ which will be observed through this investigation. Purpose: To observe and compare the reactivity of the isomers of butanol as examples of 1°‚ 2° ‚ and 3° alcohols. Hypothesis: The reactivity of primary alcohol will be lower than
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Module 7 Exam Review ANSWER KEY 1. Define acid. (7.01) An acid is a substance that produces hydrogen ions‚ H+ or hydrodium ionsH3O+ in solution. 2. Compare the three theories of acids. (7.01) An Arrhenius acid is a substance the increases the concentration of hydrogen ion‚ H+ or hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted-Lowry acid is any substance that donates a hydrogen ion‚ H+ to another substance. A Lewis acid is any substance that accepts a lone pair
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