IMG_0004_NEW_0027

IMG_0004_NEW_0027 - _ l'l dt l2'l dt Rate:Bx Rate' + rtAl...

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L5 ToDAY,S LECTURE: ..REACTION KINETICS'' . Rates and Molar Ratios . Rates and equilibrium . Pre-Equilibria . What if Forward AND Reverse reactions occur? For the elementary reactions: k, A+B =-l* Products k_1 Including Reverse Reactions Rates and Equilibrium Rates and Molar Ratios Reaction rate oC Number of molecules consumed - or produced by each reaction step . Example: For the first order reaction 2A-+28+C etAl Be careful defining the rate constant! Define fr in terms of specific reactant or product Example: We have defined the rate ofthis reaction in terms of consumption ofA We can also define the rate in terms of production of C n"t",:flld[e] =[ ate]
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Unformatted text preview: _ l'l dt l2'l dt Rate:Bx Rate' + rtAl :Elx rtAl = k=Wk, dTCl = dt F u it 5c*"nL W ) LO., 19 SanL . Reaction rate faster if concentrations are further from equilibriumconcentrations 3 k. A+B k_r Concentrations change until equilibrium is reached As defined by the equilibrium constant (K) for the reaction At equilibrium: ,t,[A][B] : f-,[Products] Equilibrium position defined by ratio of forward and reverse ,u1" "onr6n6 Q (for 2 elementary reactions) M E-RGe ft-Frsrdnac = RcY*nte At Equilibrium: Forward Reaction Rlte : Reverse Reaction Rate :+ At equilibrium: @lReaction Rate = 0 O . t "t*"u-, &hlFI *lFd-l'l...
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This note was uploaded on 12/27/2011 for the course CHEM 122 taught by Professor Williams during the Fall '10 term at Simon Fraser.

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