2013 Name : Ryan annasdass arokiasamy ID : 1206875 Group Members : Chan Pei Qie‚Chong Ven Yen Name : Ryan annasdass arokiasamy ID : 1206875 Group Members : Chan Pei Qie‚Chong Ven Yen experiment 19 kinetics : the study of a chemical reaction experiment 19 kinetics : the study of a chemical reaction Results Part A [I-] / mol dm-3 | [S2O82-] / mol dm-3 | [S2O32-] / mol dm-3 | Time /s | Rate of I2 formation / mol dm-3 s-1 | 0.2 | 0.2 | 0.01 | 1.25 | 0.1600 | 0.2 | 0.15 | 0.01
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F7 Essay Writing (Kinetics) Q. Write an essay on factors which affect the rate of reactions and discuss the uses of kinetic studies. Outlines: (I) Factors affecting the Rate of Reaction (a) temperature ---- collision of molecules with different velocities and kinetic energies ---- Collision Theory and Maxwell-Boltzmann distribution ---- Arrhenius equation and Activation energy (b) concentration ---- frequency of collisions and effective collisions
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WHAT IS TORQUE? Torque is a measure of how much a force acting on an object causes that object to rotate. The object rotates about an axis‚ which we will call the pivot point‚ and will label ’O ’. We will call the force ’F ’. The distance from the pivot point to the point where the force acts is called the moment arm‚ and is denoted by ’r ’. Note that this distance‚ ’r ’‚ is also a vector‚ and points from the axis of rotation to the point where the force acts. (Refer to Figure 1 for a pictoral
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2.6 Kinetic studies of prepared complexes The integral method of Coats–Redfern equation[19‚21‚27‚38] was used for determining the kinetic parameters of the decompositions process for the investigated metal complexes according to following equation: log[log(w_∞/(w_∞-w))⁄T^2 ]〖=log[AR/〖∅E〗^* (1-2RT⁄E^≠ )]〗-E^≠/2.303R 1/T (4) Where w_∞ is the mass loss at the accomplishment of the decomposition reaction‚ w is the mass loss at temperature T‚ ∅ is the rate of heating and R is
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Discussion Our experiment is divided into 9 parts: A. Effect of Nature of Reactants to the reaction rate. B. Effect of Temperature to the reaction C. Effect of Concentration to the Reaction Rate D. Effect of Catalyst to the Reaction Rate E. Chromate-Dichromate Equilibrium F. Thiocyanatoiron (III) Complex Ion Equilibrium G. Weak Acid Equilibrium (Ionization of Acetic Acid) H. Weak Base Equilibrium Ionization of Ammonia I. Saturated Salt (Sodium Chloride) Equilibrium On part (A) we are
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Lecture No. 1 Chemical Kinetics 1.1 The Rate of a Reaction Chemical Kinetics is the area of Chemistry that is concerned with the speed‚ rate or mechanism at which a chemical reaction occurs. Reaction Rate is the change in the concentration of a reactant or product with time (i.e. M/s). It measures how fast a reactant is consumed and how fast a product is formed. 1.2 WRITING RATE EXPRESSIONS Consider the following hypothetical reaction. A + 2B ( 3C + D Rate = - rate
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Centre Course Year/ Trimester Session : Centre for Foundation Studies (CFS) : Foundation in Science : Year 1 / Trimester 1 : 201401 Unit Code Unit Title : FHSC1014 : Mechanics Tutorial 4: Application of Newton’s Laws. 1. The distance between two telephone poles is 50.0 m. When a 1.00 kg bird lands on
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The two different types of energy are kinetic and potential energy. Kinetic energy is the energy a moving object has because of its motion. The kinetic energy of a moving object depends on the object’s mass and its speed. The kinetic energy of a moving object can be calculated from this equation: Kinetic energy (in joules) = ½ mass (in kg) x [speed (in m/s)]² KE= ½ mv² In this equation ^‚ the symbol v represents speed. Example Find the kinetic energy of the ball having mass 0‚5 kg and
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Kinetic Theory - Worksheet 1. State three (3) assumptions of the kinetic theory as it relates to gases. [3] ________________________________________________________________________ ________________________________________________________________________ ________________________________________________________________________ 2. The kinetic theory assumes that all gases are ideal‚ however‚ this does not exist in reality. a. State the conditions under which gases deviate from ideal behaviour and explain
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Kinetic Theory Objectives • Describe how the kinetic-molecular theory is used to explain how gases behave at different temperatures. (Exploration 1) • Analyze data that shows how gas particle mass affects that gas’s behavior. (Exploration 2) • Describe the Maxwell-Boltzmann Distribution. (Explorations 1 and 2) Description of Activity The kinetic-molecular theory states that a collection of gas molecules’ average kinetic energy has a specific value at any given temperature
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