01:160:162 Lecture Notes - Lecture 8: Elementary Reaction, Reaction Step, Collision Theory

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25 Jul 2017

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Collision between particles must be (cid:1445)effective(cid:1446) particles must have the necessary orientation for reaction to take place. But proper orientation may not be enough. Collision must also have enough e to overcome the activation barrier. If either of these two criteria are not met, no reaction will take place. According to collision theory, reactants must collide for reaction to occur. Some simple reactions may proceed in a single step as suggested by balanced equation for reaction ex. Reaction occurs as direct result of one effective collision of i- and ch3br. Now consider: n2 (g) + 3h2 (g) 2 nh3 (g) Highly unlikely that this reaction occurs in one step since it would require 4 molecules to collide simultaneously while all having the proper orientations. Instead, overall reaction is accomplished in simpler steps. Series of simple steps (i. e. elementary reactions) that reactants go through to become the final products of a reaction.

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61"(aq) + BrO3(aq) + 6 H+(aq) â 3 12(aq) + Br(aq) + 3 H2O lodide ions (I), react with bromate ions (BrO) with acid (H') to produce iodine (12), bromide (Br) and water. Based on the reaction, 13 particles (six I's, one BrO 's and six Hs) all must somehow collide, hold on to each other, and react. The probability is highly unlikely, a more realistic scenario is for the reaction to take place in a series of collisions, each one involving two or three particles, each one resulting in part of the reaction taking place. This is one of the purposes behind the study of rate laws establishing the sequence of events occurring during the transformation of reactants into products. This sequence of events is called a reaction mechanism. The order of the reaction of I, BrO and H will be calculated in this experiment. The results from this experiment will be used to calculate the energy of activation in the next experiment. The reaction has the rate law: The initial rate method will be used to determine the order of each reactant (the values of x, y, and z). In this method, the reaction is clocked as it proceeds for only a small portion of the total time it would take to reach completion. The time the reaction is measured during the first 5% or so of the reactants being consumed. Each experimental trial will change the concentrations of one of the other concentrations remain unchanged. compounds while the Rxn l : 6 I(aq) + BrO3(aq) + 6 H+(aq) â 3 12(aq) + Br(aq) + 3 H2O The timing method you will use is based on the properties of one of the products of the reaction, the I2 molecule. Two reactions that the 2 molecule can undergo in this experiment are: (a fast reaction) Rxn 2: 3 12 (aq) + 3 starch â deep blue complex Rxn 3: 3 12(aq) + 6 S,032-(aq) â 6 I(aq) + 3 S,062-(aq) (a very-fast reaction) (The stoichometry of Rxn's 2 and 3 have been adjusted to match the 3 moles of h produced in Rxn 1.) The reaction to be studied is rxn. As the reaction proceeds it creates iodine (2). The iodine created will quickly react with S2Os (thiosulfate ion) via rxn 3. Rxn 1 wil continue to produce iodine and the iodine will quickly react with thiosulfate al of the thiosulfate has reacted. Once all of the thiosulfate has reacted, the iodine produced will now react with starch via rxn 2. The reaction with starch produces a blue color. The rate of the reaction can now be timed and triggered by the appearance of a blue color and can be directly calculated as Î[S20321 The rate of Rxn 1 can now be correlated to the rate of Rxn3

01:160:162 Lecture Notes - Lecture 8: Elementary Reaction, Reaction Step, Collision Theory

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