...Investigación y Desarrollo de Educación Bilingüe Biology I INTEGRATIVE ACTIVITY 1 SCIENTIFIC METHOD Teacher: Ms. Nashiely Moreira Diana Paola Amaro de la Paz Marco Bautista Cerda Ricardo Bazán Godoy Katia Paola Aguilar Tamez Verónica Gabriela Aranda Holguín Oxidation of a Fruit Introduction: The topic of this project is about the oxidation of the fruit when they are exposed to the air, and how the ascorbic acid (Vitamin C) is effective in preventing oxidation. First of all, oxidation is caused because, in some tissues exist enzymes that reacts with the oxygen, and it causes the oxidation of some components of the cells. These enzymes cause the dark coloration that has the fruits when they are exposed to the air. But some substance, like ascorbic acid, well known as Vitamin C, prevents that the oxygen reacts with the enzymes, and then it could slow down the aging of the tissues. Problem: The oxidation of a fruit exposed to air, can be controlled? With this controlled experiment, we are looking for substances that could slow down the aging of the fruit’s tissues, so we could prevent the oxidation of it. Hypothesis: We believe that if we add Vitamin C to a fruit, it could slow down the oxidation of the fruit. Controlled experiment Materials: 3 plastic containers 1 apple Water Ascorbic acid (Vitamin C) 1. Cut three little pieces of the apple. 2. In the first container put one piece of the apple 3. In the second container put another piece...
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...Temasek Secondary School Secondary 4 Pure Chemistry Test Practice 3 15 Topic: Reduction & Oxidation Parent’s signature and comments: ……………………………………………………………………………………………………. Name: Class: Register No: Sec 4/ Date: / 02 / 2016 Section A (3 marks) Each question below is provided with four answers. Select the most appropriate answer and fill it in the brackets provided. 1. Iron metal is extracted from iron(III) oxide through a series of reactions in a blast furnace. The five reactions that occur in the blast furnace are: Reaction 1: C + O2 CO2 Reaction 2: CaCO3 CaO + CO2 Reaction 3: CO2 + C 2CO Reaction 4: Fe2O3 + 3CO 3CO2 + 2Fe Reaction 5: CaO + SiO2 CaSiO3 Which of the above reactions are not redox reactions? A 1 and 3 only B 2 and 5 only C 1, 2 and 5 only D 3, 4 and 5 only ( ) 2. The nickel-cadmium rechargeable battery is based upon the following overall reaction. Cd + 2NiO(OH) + 4H2O Cd(OH)2 + 2Ni(OH)2.H2O What is the oxidation number of nickel at the beginning and at the end of the reaction? 1 beginning end A +1.5 +2 B +2 +3 C +3 +2 D +3 +4 ( ) 3. When substance X is added to aqueous potassium iodide and acidified potassium manganate(VII) solution separately, both resultant solutions appear colourless. In the two reactions, substance X is acting as A an oxidising agent only. B a reducing agent only. C both an oxidising agent...
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...Week Seven Lab Discussion Each team member completed an oxidation-reduction lab during week six. The team members then shared their findings with each other for comparison and discussion. The purpose of this lab was to determine relative oxidizing and reducing strengths of a series of metals and corresponding ions. Oxidation and reduction reactions occur simultaneously. In oxidation, electrons are given, and in reduction, electrons are gained. An oxidizing agent is a chemical substance, which has a large tendency to gain electrons, while a reducing agent is an element, which loses electrons to another chemical species and is therefore oxidized. This lab used metals and provided substances to determine reactions. These results were recorded in a data table and the results were analyzed based on these observations. These results were used to help the team gain a better understanding of the reactions between the metals and the solutions. Discuss and Compare End-of-Lab Questions Data Table Results: Magnesium (Mg) in sodium sulfate (Na2SO4): three team members observed bubbling, two stated that they observed no reaction, and one observed only a slight reaction. Zinc (Zn) in magnesium sulfate (MgSO4): no team members observed a reaction. Lead (Pb) in zinc nitrate (Zn(NO3)2: five members did not observe a reaction, while one member noted and removed a layer of tarnish, and last member stated that it formed a clear coating on the lead. Lead (Pb) in iron (III) chloride...
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...Sharif Mursal PSY/202 Instructor: Sharon Clark Assignment: Adolescence and Adulthood September 15, 2013 Axia Collage University of Phoenix The psychosocial development stage during adolescence is the search for identity. Psychosocial development encompasses the way peoples understanding for themselves, one another and the world around them changes during the course of development. I think that around the age of 15 years old I was starting to go through this stage. I got my first part time job and no longer sensed that I needed my parents to give me the money to go and do what I wanted. If I didn’t need their money I imagined that they couldn’t tell me what I could or could not do. Being that I was doing the things my parents asked me not to do, such as hang out with older guys, I began sensing pressured into doing things I wouldn’t have otherwise tried at the young age of 15 years old. This made me feel that I was capable to better adequate in with this specific crowd I surrounded myself with. I dabbled with alcohol, drugs which hastily became an almost every day thing later leading me into a life of alcoholism and addiction. These are things I wish I could go back and change but have also shaped me into being the person I am today. For that I am thankful to God because I have gained remarkable life experience in the progression. In late adulthood there are some physical and reasoning changes that happen. Some of the physical variations brought about by the maturing...
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...Experiment 34A: Hypochlorite Oxidation of Methyl Ketones by the Haloform Reaction: Benzoic Acid Objective: To practice the Haloform reaction as synthetic rout to form benzoic acid To understand the mechanis that provide chorine from NaOH To obtain the melting point and FTIR spectrum of benzoic acid Experimental Procedure: The procedure was followed as described in Mayo, pages 405 -406, with the modifications given on Blackboard. Additional modifications to the procedure included the following: * The filtered product was left on the Hirsch funnel for 1 5 min * The amount of Na2SO3 was increased from 15 to35 mg * The amount of Acetophenone was increased from 15 to35 mg * The amount of Na2SO3 was increased from 90 μL, from 60 μL. * The amount of Sodium hypoclorite was increased to 3.2 mg Reaction scheme Data and Results: Physical properties Compound | Formula | MW | Amount | mmol | Mp 0C | Bp 0C | d | nD | Acetophenone | C₆H₅COCH₃ | 120.16 | 90 μL. | 77 | 20.7 | 2.2.6 | 1.03 | 1.5372 | Aquous NaOCl | NaOCl | 74.442 | 3.2mL | | 18 | 101 | 1.11 | | Sodium sulfite | Na2SO3 | 120.6 | 35mg | | | 33.4 | | | Benzoic acid | C6H5COOH | 122.12 | 94mg | 77 | 121.0 | 249 | | | Chloroform | CHCl3 | 119.38 | 92mg | | | | | | Water | H2O | 18.015 | 1.5mL | | 32 | 100 | 1.00 | | Observations: * Acetophenone and NaOCl were clear liquids * Sodium Sulfite was a whote powder * A yellow greasy liquid was found at the...
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...Experiment 5 Enzyme Kinetics: The Effect of Yeast Alcohol Dehydrogenase and Coenzyme on the Rate of Oxidation of Ethanol. Results Raw data: Effect of Enzyme Concentration | Reagent | 1 | 2 | 3 | 4 | Buffer B | 2.5 ml | 2.4 ml | 2.3 ml | 2.2 ml | NAD+ | 200 μl | 200 μl | 200 μl | 200 μl | Dilute ADH | 200 μl | 300 μl | 400 μl | 500 μl | 6 M Ethanol | 100 μl | 100 μl | 100 μl | 100 μl | Time 0 sec. | 0.022 | 0.026 | 0.069 | 0.073 | Time 5 sec. | 0.028 | 0.038 | 0.110 | 0.114 | Time 10 sec. | 0.038 | 0.051 | 0.141 | 0.150 | Time 15 sec. | 0.048 | 0.064 | 0.176 | 0.187 | Time 20 sec. | 0.058 | 0.078 | 0.206 | 0.222 | Time 25 sec. | 0.068 | 0.091 | 0.239 | 0.259 | Time 30 sec. | 0.078 | 0.104 | 0.270 | 0.291 | Time 35 sec. | 0.088 | 0.115 | 0.301 | 0.325 | Time 40 sec. | 0.099 | 0.131 | 0.331 | 0.358 | Time 45 sec. | 0.109 | 0.145 | 0.362 | 0.391 | Time 50 sec. | 0.119 | 0.158 | 0.392 | 0.424 | Time 55 sec. | 0.130 | 0.167 | 0.420 | 0.455 | Time 60 sec. | 0.140 | 0.179 | | | Effect of Coenzyme(NAD) Concentration | Reagent | 1 | 2 | 3 | 4 | Buffer B | 2.4 ml | 2.35 ml | 2.3 ml | 2.25 ml | NAD+ | 10 μl | 50 μl | 100 μl | 150 μl | Dilute ADH | 500 μl | 500 μl | 500 μl | 500 μl | 6 M Ethanol | 100 μl | 100 μl | 100 μl | 100 μl | Time 0 sec. | 0.009 | 0.020 | 0.032 | 0.102 | Time 5 sec. | 0.015 | 0.038 | 0.049 | 0.152 | Time 10 sec. | 0.023 | 0.056 | 0.068 | 0.190 | Time 15 sec. | 0.029 | 0.072 | 0.088 | 0.229 | Time...
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...In that example, the iron is oxidized and the oxygen is reduced. Reduction is the opposite of oxidation. A reduction reaction always comes together with an oxidation reaction. Oxidation and reduction together are called redox. Oxidation is a gain of oxygen. Reduction is a loss of oxygen. For example: * Fe2O3 + 3CO → 2Fe + 3CO2 Both reduction and oxidation go on at the same time which is a redox-reaction. The gain of Hydrogen-atoms; and, the simultaneously loss of oxygen-atoms, is known as reduction. Oxidising agent is a chemical that releases oxygen atoms. For example, potassium chlorate has a chemical formula of KClO3. When it oxidizes a reducing agent, such as powdered aluminium metal, it loses its oxygen to the aluminium and becomes potassium chloride, KCl. It is also referred to as a chemical that accepts electrons from a reducing agent. For example, potassium permanganate has an oxidation state of +7. In acid solution, it gains 5 electrons (e-), becoming a manganese compound with an oxidation state of +2. Most oxidizing agents of the second (electron-accepting) definition have oxygen, but not all. For example, fluorine (F2), the most powerful oxidizing agent, does not have any oxygen in it. When it acts as an oxidizing agent, it gains an electron to transfer from an oxidation state of 0 to an oxidation state of -1. Combustion is a type of oxidation-reduction reaction and hence it is a redox reaction. An explosion is a fast form of combustion...
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...as in a battery, it is an electrochemical reaction. In contrast, chemical reactions where electrons are transferred between molecules are called oxidation-reduction (redox) reactions. In general, electrochemistry deals with situations where redox reactions are separated in space or time, connected by an external electric circuit. Principles Oxidation and reduction The term "redox" stands for reduction-oxidation. It refers to electrochemical processes involving electron transfer to or from a molecule or ion changing its oxidation state. This reaction can occur through the application of an external voltage or through the release of chemical energy. Oxidation and reduction describe the change of oxidation state that takes place in the atoms, ions or molecules involved in an electrochemical reaction. Formally, oxidation state is the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic. An atom or ion that gives up an electron to another atom or ion has its oxidation state increase, and the recipient of the negatively charged electron has its oxidation state decrease. For example, when atomic sodium reacts with atomic chlorine, sodium donates one electron and attains an oxidation state of +1. Chlorine accepts the electron and its oxidation state is reduced to −1. The sign of the oxidation state (positive/negative) actually corresponds...
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...5. At the bare GCE, there is nearly nothing in the voltammogram but a very small oxidation peak was observed at 0.52 V for oxidation of ceftazidime at GCE modified with PDPA. The current increased at MWCNT/GCE and MWCNT-β-CD/GCE. However, the further increasing MWCNT-β-CD/PDPA/GCE was seen due to synergistic effects of MWCNT and PDPA and also peak potential shifted to more negative potential (0.51 V) but the most current was seen at MWCNTs-β-CD-OPDPA/GCE. These variations showed that the MWCNTs-β-CD-OPDPA/GCE not only combines high conductivity and electrocatalytic effect of MWNTs and also PDPA with the ability of β-CD to form inclusion complexes with ceftazidime but also the ability of the oxidized polymer for increasing of current. These facts and also diminished background current or oxidized polymer cause to the best analytical features and the...
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...Alkanes Preparation: 1. Hydrogenation of alkenes 2. Hydrogenation of alkynes 3. Reduction of alkyl halides 4. Coupling of alkyl halides (Wurtz reaction) 5. Hydrolysis of Grignard reagent Reaction: 6. Oxidation 7. Halogenation Cycloalkanes Preparation: 1. Carbene insertion 2. Simmons-Smith reaction 3. Modified Wurtz reaction 4. Dieckmann condensation Reaction: 5. Opening reactions of three- and four-membered rings 6. Halogenation 7. Oxidation Alkenes Preparation: 1. Dehydrohalogenation of alkyl halides (E2 Elimination) 2. Acid-Catalyzed Dehydration of alcohols 3. Dehalogenation of vicinal dihalides Reaction: 4. Halogenation 5. Hydrohalogenation 6. Addition of HBr in Peroxide 7. Hydration 8. Oxymercuration-Demercuration 9. Hydroboration-oxidation 10. Catalytic hydrogenation 11. Epoxide formation 12. Oxidation 13. Ozonolysis cleavage 14. Cationic polymerization 15. Free-radical polymerization 16. Addition of halogens and water (Halohydrin formation) Alkynes Preparation: 1. Dehydrohalogenation of vicinal and germinal dihalides 2. Dehalogenation of vicinal tetrahaloalkanes 3. Substitution Reaction: 4. Hydrogenation 5. Hydrohalogenation 6. Halogenation 7. Hydration (keto-enol tautomerization) 8. Reaction of acidic terminal hydrogen (acid-base reaction) Alkyl Halides Preparation: 1. Addition of halogen...
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...→ Fe3+ + OH- Also, Fe3+ ions formed can consume H2O2 to generate Fe2+ and hydroperoxyl radicals (HO2.). Therefore, higher Fe2+ concentration has got less significance for the oxidation reaction as this becomes detrimental to COD removal (Loures et al. 2013). Figure 5: Effect of Fe2+ concentration on COD removal during pre-treatment of landfill leachate by Fenton oxidation. Effect of different strength of landfill leachate on treatment by Fenton process Strength of landfill leachate was varied to increase the efficiency of Fenton oxidation, this was done to assess the influence of dilution, for instance, if landfill leachate are co-treated with municipal wastewater. COD concentration was varied by diluting landfill leachate with tap water. Fig.6 shows that COD removal efficiency increased from 94% to 98% when landfill leachate was diluted 30 times. Therefore, after diluting the landfill leachate efficiency of COD removal by Fenton process increased by 4%. Maximum COD removal was achieved at 30 times initial dilution of leachate which gave an initial COD of 240 mg/L and final COD after treatment...
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...Experiment 8: Redox: Analysis of the Oxidizing Capacity of Bleach PURPOSE In this experiment, you will show how redox reactions can be used to quantitatively determine the amount of oxidizing agent in liquid hypochlorite household bleach. There are two oxidation-reduction reactions for determining the oxidizing capacity of bleach. Initially an excess of iodide ions are added to a bleach solution. The iodide ions are oxidized to iodine after the solution has been acidified. Starch is added to the resulting iodine solution as an indicator. The solution is then titrated with sodium thiosulfate until the color of the solution changes indicating the endpoint of the reaction. Data collected from the titrations will be used to calculate the mass of the sodium hypochlorite in an unknown solution of bleach. Given the original mass of the unknown solution and the calculated mass of the sodium hypochlorite in the unknown solution, the percent by mass of the sodium hypochlorite can be determined. The oxidizing capacity of the unknown bleach is effectively the percent by mass of the sodium hypochlorite in the unknown bleach sample. OJECTIVES 1) Titration of a sample of bleach with thiosulfate. 2) Determining the end point of the titration with starch indicator. 3) To determine oxidizing capacity of bleach by determining the percentage by mass of the bleach that is sodium hypochlorite. 4) Balance and summarize the two redox reactions to determine the overall chemical reaction that...
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...Tomas Abstract: In this experiment, we used dry cell battery. The two main objectives of the experiment are to (1) relate and apply the concepts of electrochemistry to actual experiments, (2) understand the processes and elements of an electrochemical cell and (3) determine the spontaneity of reduction-oxidation (redox) reactions based on standard reduction potential. Different half-cells were prepared and connected to copper, which served as the reference electrode, to set up a voltaic cell. The volt-meter readings of the set-ups were then used to calculate for the standard reduction potentials of the variable half-cells. The results obtained from the experiment indicated the spontaneity of the redox reactions investigated, showing that the least spontaneous system is that connected to another copper half- while the most spontaneous system is that connected to the Zinc half-cell. Introduction: Electrochemistry is the study of the relationships between chemical reactions and electricity. The functionality of every portable electronic device you own, whether it be your laptop, Ipod, or cell phone, is made possible by electrochemical reactions. Fundamental oxidation/reduction reactions occur inside the batteries of these devices. Chemists and engineers all over the world are searching for ways to improve the technology by developing materials, which will make the batteries for these devices cheaper, more lightweight, and longer lasting. Electrochemical reactions can be spontaneous...
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...the meaning of the term oxidation state. ..................................................................................................................................... (1) (c) Complete the table below by deducing the oxidation state of each of the stated elements in the given ion or compound. |Oxidation state| Carbon in CO|| Phosphorus in PCl|| Nitrogen in Mg3N2|| (3) (d) In acidified aqueous solution, nitrate ions, NO, react with copper metal forming nitrogen monoxide, NO, and copper(II) ions. (i) Write a half-equation for the oxidation of copper to copper(II) ions. ........................................................................................…............................... (ii) Write a half-equation for the reduction, in an acidified solution, of nitrate ions to nitrogen monoxide. ........................................................................................…............................... (iii) Write an overall equation for this reaction. ........................................................................................…............................... (3) (Total 8 marks) 5. (a) The following is an equation for a redox reaction. 2NO + 12H+ + 10I– ® 2NH4+ + 2H2O + 5I2 (i) Define oxidation in terms of electrons. ..................................................................................................................... (ii) Deduce the oxidation state of nitrogen in NO...
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...Answer the questions below. When you have finished, submit this assignment to your teacher by the due date for full credit. (8 points) Score 1. The diagram shows an electrochemical cell with a copper strip in a solution of copper (II) sulfate (left) and a magnesium strip in a solution of magnesium sulfate (right). In your response, do the following: • Label all parts (1–9), including the solutions in each beaker and the connecting tube. 1 electrode (cathode). 2. Copper solution 3. Cell for Reduction 4. Voltmeter (Light Bulb) 5. Cell for Oxidation 6. Magnesium Solution 7. Wire (conductor) 8. Electrode (anode) 9. Salt Bridge • Label which cell is the cathode and which cell is the anode. Include the charge on each strip....
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