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Chemistry 1302A/B Lecture Notes - Lecture 15: Chemical Kinetics, Reaction Rate, Reaction Rate Constant

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harlequinbadger850

30 Dec 2018

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Western University

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Course

Chemistry 1302A/B

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Document Summary

Chemical kinetics is the study of how quickly a reaction will proceed. The study of the rate at which a reaction will proceed relative to time. There are many factors that infulence the rate of the reaction. To name a few, these are concentration, temperature and catalysts. In this chapter we will be looking at these factors and some laws that affect the rate. The rate of a chemical reaction is usually defined by comparing the change in the product (or reactant) concentraion over time. N2 + 3h2 -> 2nh3 one could measure the rate at which either n2 or h2 is consumed relative to time or the rate at which nh3 is produced relative to time. Due to the stoic, we know that the rate of n2 consuption will be 1/3 the rate of consuption of the h2 consuption and 1/2 the nh3 production.

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Related Questions

Did the reaction actually stop when the blue-black color appeared? Explain briefly

EXPERIMENT 16 A Kinetic Study of an Iodine Clock Reaction OBJECTIVES: To measure experimental reaction rates under different conditions. To use the method of initial rates to determine the order of reaction. To determine the rate constant of a reaction at different temperatures. To determine the activation energy of a reaction using graphical techniques. rate law. To make deductions regarding a reaction mechanism, based on the INTRODUCTION: According to chemical kinetics, it is possible to write down a Rate Law' for any chemical equation: Rate k[A]m [B] This rate law can be used to calculate the rate at which that particular reaction will proceed when a given concentration' of [A] and [B] are present in the system. However, to do this we must know the value of (it is temperature dependent). k rate constant m order with respect to concentration of A. n order with respect to concentration of B. It is important to realize that the values of k, m and n cannot be determined by looking at the chemical equation. They must be deduced experimentally someone must actually run and time the reaction under varying conditions. In this lab, we will studythe Rate Law forthe following reaction between the persulfate ion,s2os and the iodide ion. General Rate Lane. Rate -k ]m [s20g2-1n This reaction is called a clock reaction b of the thiosulfatestarch indicator system we use to time the reaction. Every you run this reaction, your flask will contain an indicator system consisting of time 5.0 x 105 moles of thiosulfate' ions, S2032, and a little starch. When the two reactants, Ose are first mixed start the reaction, every molecule of I2 that is produced reacts immediately with any nt according to the following chemical equation. S2032-preset 21- S40 12 2 S203 This removes the first 2,5 x 10 s moles I2 (look at stoichiometry of reactions above) from the system but then the thiosulfate is gone. This point is marked by the almost instantaneous appearance of an intense blue-black Also called Rate Equation and Rate Law Expression square brackets around anything, [X], means moles per liter of Xor molarin of x. You pipet 100 ml of 0.0050 M Naasio, into each flask.

Please answer both questions. They are part of one question in a pre lab. I have attached the introductory statement referred to in the first part. Thanks!