The Formation of Alum Experiment 4 Introduction In an increasing population the need for land fields are as well increasing daily. Better yet‚ rather than dumping off trash is to instead recycle aluminum cans for a more efficient society. In this lab we will show how aluminum cans react to form alum. Materials and Methods The first step of the lab is to measure the mass of 250 mL beaker‚ once you have done this add .9 to 1.2 grams of aluminum can pieces to the beaker. Take the mass once
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Chemical Kinetic Models Simplified Global Chemical Kinetic Model In order to compare the two reactors used in our experiment‚ a simplified global kinetic model was used to describe the DRM reaction behavior in different plasma reactor. This model was already used by authors in the field of pollutant removal by using a plasma reactor [15‚ 21–23]. It is generally accepted that free radical processes are the main mechanisms in non-equilibrium plasma reaction [21‚ 24-25]. The chemical kinetics model
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Linear Regression & Best Line Analysis Linear regression is used to make predictions about a single value. Linear regression involves discovering the equation for a line that most nearly fits the given data. That linear equation is then used to predict values for the data. A popular method of using the Linear Regression is to construct Linear Regression Channel lines. Developed by Gilbert Raff‚ the channel is constructed by plotting two parallel‚ middle lines above and below a Linear Regression
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Department of Electronics and Communication Engineering AU College of Engineering (Autonomous) Scheme of Instruction‚ Examination and Syllabus B.E. (Electronics and Communication) – 4 Year Degree Course Common Scheme of Instruction & Examination I/IV B.E./B.Tech (Four Year Course) – Semester System (with effect from 2006 – 2007 admitted batch onwards) First Year I & II Semesters Code No. ENG 1001 ENG 1002 ENG 1003 ENG 1004 ENG 1005 ENG 1006 ENG 1007 ENG 1008 ENG 1009 ENG 1010 ENG 1011 ENG 1012
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investigate reaction rates‚ and it is a reaction between acidified hydrogen peroxide and potassium iodide: 2H+(aq) + 2I¯ (aq) + H[-1] 2O2 (l) ÕI2 (aq) + 2H2O2 (aq) Iodide ions are firstly oxidised by the hydrogen peroxide‚ as shown in the above equation. The iodine that is then produced reacts immediately reacts with thiosulphate ions as follows: I2 (aq) + 2Na2S2O3 (aq) Õ 2NaI (aq) + Na2S406 (aq) As soon as all of the thiosulphate ions have reacted with the iodine‚ the excess iodine
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CHEMISTRY (Theory) Time allowed : 3 hours General Instructions: (i) All questions are compulsory. Maximum Marks : 70 (ii) Marks for each question are indicated against it. (iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark each. (iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks each. (v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks each. (vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks
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[I-]x [H2O2-]y where k is the rate constant‚ x and y are the orders‚ and the rate is equal to rate [I2]/t. Once the rate law is determined‚ the activation energy can be calculated using the Arrhenius equation. By using logarithms‚ the Arrhenius equation can be converted into the following linear equation: k = Ae-Ea/RT ln k = ln A- Ea/RT slope = -Ea/R Procedures: After following the usual lab rules and wearing personal protective equipment‚ we began by measuring out our solutions. Next we prepared
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CHM1051 Chemistry CHM1051 has been designed for students who have demonstrated a strong aptitude for chemistry during secondary studies‚ eg. a VCE Chemistry Study Score >=37. On completion of this unit‚ students will have gained an understanding of how atoms and molecules interact with each other and how this affects their bonding‚ reactivity‚ 3D structure and physical properties. A number of important topics such as stoichiometry‚ intermolecular forces‚ thermodynamics‚ kinetics‚ equilibria‚
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reactant or the rate of increase of the concentration of a product. The rate law is an equation that expresses the rate of a reaction as a function of the concentration of all the species present in the overall chemical reaction at some time. The rate law is often found to be proportional to the concentration of the reactants raised to a power. For the depolymerization of diacetone alcohol the empirical rate equation is -∂x∂t=kxn[OH-]m (1) X= concentration of diacetone alcohol ‚ t=time ‚ k=rate
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* 9/4/12 12.3 - crystal structures crystalline structure: possess rigid and long-range order; its atoms‚ molecules‚ or ions occupy specific positions (Exs. wax ‚ice‚ sugar‚ salt‚ diamond‚ etc.) unit cell: basic repeating structural unit of crystalline solid -there are seven types of unit cells coordination number: number of atoms surrounding an atom in a crystal lattice -higher coordination number --> more tightly packed structure 3 types of cubic unit cells: -primitive cubic (sc) c#:
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