color or tone of the light spectrum. Materials: Several materials were needed for the conduction of this experiment. Bunsen burners were used to generate heat. The process also required elements in liquid state‚ LiCl‚ NaCl‚ KCl‚ CaCl2‚ SrCl2‚ CuCl2‚ BaCl2‚ nichrome wire(or remove a pre-soaked wood splint)‚ small test tubes for the metal ion solutions‚ safety goggles‚ and tabs to absorb the liquids. Containers were labeled to identify each element. Observations were recorded on a data table.
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The goal for this experiment is to determine which out of the four balanced chemical equations best represent the thermal decomposition of sodium bicarbonate. The guiding question will be answered with the outcome of the sodium bicarbonates thermal decomposition and it being plugged in into the four balanced chemical equations. John Dalton atomic theory explains two fundamental laws of chemistry which are the law of conservation of mass and the law of definite proportions. The atomic theory states
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Introduction: Copper (II) Chloride is the compound with a chemical formula of CuCl2. This is a light brown solid‚ which slowly absorbs moisture to form a blue green dihydrate. Copper (II) Chloride is highly soluble in water and will produce a blue solution. solutioAluminum is the compound that has a chemical formula of Al. This is a silver solid that can be easily formed‚ machined‚ or cast. In this lab‚ we will be finding the limiting reactant between Copper(II) Chloride and Aluminum. The limiting
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Topics and Concepts Covered Topics covered are suggested by the College Board. The order of presentation is strongly recommended by the National Mathematics and Science Initiative (NMSI) UNIT 1 Foundations / Nomenclature / Stoichiometry (Summer Work and Introductory Review) these topics are all covered in College Prep and Honors Chem Chapter 1 Introduction: Matter and Measurement 1.1 The Study of Chemistry The Atomic and Molecular Perspective of Chemistry 1
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Finally we weighed the filter paper and recorded the mass in our data table. Our result for this lab was that both total product and the mass of the total reactants was 2.71g we had a 2.5 difference. This shows that we did not validate the stoichiometry of mass. That we lose moles or it’s mass. The physical changes in this lab were that the blue copper rocks changed to blue liquid. The Error we faced in this lab was that copper residue did not end up in the filter paper. II. Objective
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ORIGINAL ARTICLE The use of the stable free radical diphenylpicrylhydrazyl (DPPH) for estimating antioxidant activity Philip Molyneux Abstract Molyneux‚ P. The use of the stable free radical diphenylpicrylhydrazyl (DPPH) for estimating antioxidant activity Songklanakarin J. Sci. Technol.‚ 2004‚ 26(2) : 211-219 The use of the stable free radical diphenylpicrylhydrazyl (DPPH) to estimate the activity of antioxidants is reviewed. Current applications of the method are examined‚ particularly
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Basic Stoichiometry PhET Lab Let’s make some sandviches! Introduction: When we bake/cook something‚ we use a specific amount of each ingredient. Imagine if you made a batch of cookies and used way too many eggs‚ or not enough sugar. YUCK! In chemistry‚ reactions proceed with very specific recipes. The study of these recipes is stoichiometry. When the reactants are present in the correct amounts‚ the reaction will produce products. What happens if there are more or less of some of the reactants
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EXPERIMENT 1 IDENTIFICATION OF UNKNOWN COMPOUNDS Date of experiment : 7th August 2012 Venue: ME204 INTRODUCTION Chemical reactions are regularly categorized into 3 types: oxidation-reduction (redox reaction)‚ precipitation (double displacement) and acid-base reaction (double displacement) Type 1: Oxidation-Reduction Reactions Oxidation-reduction processes include the movements of electrons form oxidants to reductants‚ which lead to increases in oxidation
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Name: Exp 9: Stoichiometry of a Precipitation Reaction Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 CaCl2.H2O(aq)= m/M =1/147 =0.0068 mol CaCO3(s)=0.0068*1/1 =0.0068 mol CaCO3 (s)= CaCO3 mol *CaCO3 g =0.0068 mol*100.01 g =0.68 g Convert moles of Na-2CO3 to grams of Na2CO3 = 0.00680 moles Na-2CO3 x 105.99g Na-2CO3 1 mole Na-2CO3 = 0.72g 0.72g of Na-2CO3 to fully react with 1g of CaCl2-.2H2O Step 4: Mass of weighing dish
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Lab: STOICHIOMETRY The reaction of Iron with Copper(II) Sulfate Purpose: In this experiment we will use stoichiometric principles to deduce the appropriate equation for the reaction between metallic iron and a solution of copper (II) sulfate. This reaction produces metallic copper‚ which is seen precipitating as a finely divided red power. Materials: Flask beaker Copper solution Balance Hot plate •150 ml beaker •1 gram of iron power
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