Mechanism of Catalytic Cracking 11 2.6 Kinetic and modeling for catalytic cracking 14 3. Characterization and Analysis techniques 15 3.1 catalyst characterization methods 15 3.1.1 XRD 15 3.1.2 BET 15 3.1.3 SEM 15 3.2 bio mass and bio oil analysis methods 15 3.2.1 TGA (Thermo-gravimetric analysis) 15 3.2.2 FT-IR 16 3.2.3 GC-MS analysis 16 4. Experimental and modeling studies on wheat strew biomass 17 4.1 Sample measurement 17 4.2 Kinetic modeling 18 4.3 Data calculation 22
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| | Kinetics Author: Katie Wood Instructor: Donald Kavanagh Chem 106b‚ Section 001 Lab Performed 8th‚ 2012 Lab Report Submitted February 22nd‚ 2012 Abstract The purpose of the lab was to determine the order of reaction for the dye Red #40. By measuring the reaction rate between bleach and the dye‚ the order of the reaction was determined to be first order. Introduction The study of kinetics is important for studying the amount of time it takes for a particular reaction to reach
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Observations of Chemical and Physical Change PART 1 – OBSERVATIONS OF CHEMICAL CHANGE No credit will be given for this lab report if the Data section is not completely filled out and if the required photographs are not received. At least one photograph must show the student’s face. OBJECTIVES 1. Observe physical and chemical changes. 2. Define physical and chemical change. 3. Identify the relationship between a chemical change and a chemical reaction. 4. Observe several indicators of a chemical reaction
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minutes. 4. a) The hydrogen peroxide is used up and the manganese dioxide remains unchanged. Part two Title: Enzyme Function Purpose: To observe the role of enzymes in chemical reactions and to determine the kinds of cells that contain more of the enzyme catalase. Prior Knowledge: Enzymes are proteins that assist the chemical reactions of a cell by lowering the amount of activation energy needed to start the reactions‚ thereby enabling the cell to carry out the reactions at a faster rate; enzymes
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Kinetics Kinetics 6.1 Rates of reaction 6.2 Collision theory 6 16.1 Rate Expression (AHL) 16.2 Reaction mechanism (AHL) 16.3 Activation energy (AHL) 6.1 Rates of reaction 6.1.1 Define the term rate of reaction. 6.1.2 Describe suitable experimental procedures for measuring rates of reactions. 6.1.3 Analyse data from rate experiments. © IBO 2007 Figure 601 An explosion is a quick reaction D ifferent chemical reactions occur at different rates (i.e. speeds)
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reaction orders‚ and half-life of a reaction. The reaction of interest is the addition of a hydroxyl group to the nucleus of Crystal Violet. Crystal Violet‚ or hexamethylparaosaniline chloride for short‚ is a strongly colored purple dye with the chemical formula C25H30N3Cl and disassociates completely in solution. The relevant structure for this compound can be seen in figure 1 Figure 1 The base that is being used for the reaction is the strong base Sodium Hydroxide‚ or NaOH. This molecule
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Case 3: The Grayson Chemical Company The Company The Grayson Chemical Co. manufactured industrial chemicals for sale to other industrial companies. The company was about 40 years old and had been run by a stable management under only two presidents. Within the past few years‚ however‚ declining earnings and sales had brought pressure from the board of directors‚ investment bankers‚ and stockholder groups to name a new president. The company had grown increasingly stagnant – although at Grayson
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collide and bounce off each other‚ transferring energy among themselves when the collide. In order for a reaction to occur‚ there must be collisions between molecules. Through experimentation‚ factors are discovered that influence the reaction rates of chemical reactions include the concentration of reactants‚ temperature‚ surface area‚ the physical state of reactants‚ and a catalyst. This experiment regarding the factors that affect reaction rate tests the effects of increased concentration and temperature
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Submitted to: DR ISRAR AHMED CHEMICAL KINETICS Chemical kinetics is the branch of chemistry which deals with the study of the rate of reactions‚ the factors affecting the rate of reaction and mechanism of the reaction. These factors may be concentration‚ pressure‚ temperature‚ surface area‚ catalyst etc. Types of chemical kinetics: Chemical kinetics can be divided into two types: 1. Homogeneous kinetics. 2. Heterogeneous kinetics. The branch of chemical kinetics which deals with the study of
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reaction between peroxodisulphate ion S2O82-‚ and iodide ion‚ I-. S2O82-(aq) + 3 I-(aq) --> 2 SO42-(aq) + I3(aq) The general expression for the rate law‚ given this overall reaction‚ is: rate of disappearance of S2O82- = k[S2O82-]m[I-]n Chemical Kinetics is the chemistry of how fast or slow something is. These rates of reaction or the speed depends on many factors. Experiments show that the rate of homogenous reactions depend upon: The nature of the reactants‚ the concentration
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