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Lecture 4

CHEM102 Lecture 4: Chem 102 Lecture 4

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Sai Yiu

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Chem 102 Lecture 4 Monday, January 15, 2018 Zero order reactions [A] = - kt + [A0 Dont need to memorize it The trend is usually a linear line that goes down Half-life The half-life of a reaction is the time required for a reactant so that half its original concentration is reacted t1/2= [A]0/ 2k Half-life of zero is dependent on the initial concentration First order reactions aA products ln[A] = -kt + ln[A0 ln[A] = natural log of concentration of A at time t ln[A] 0 natural log of initial concentration of A Another form of first order integrated rate law [A] = [A]0e -kt Half-life for first order reaction is constant What can we say about the half-life of first-order reactions? o Half-life of A is always 24 minutes o For first-order reactions, half-life is independent of initial concentrations From the half-life of a first-order reaction, the rate constant, k, can be determined Homework question Do 1, then substitute that into 2 and 3 Second order reactions Note: you do not need to memorize formulas, but you need to know which formula is used for what purpose 1/[A] versus time, t Reciprocal of the [A], then the reciprocal of the initial concentration First half-life is short, second one is longer, third one is even longer Half-life is dependent (inversely proportional) on initial concentration Summary First order: k=[A] Second order: k=[A] 2 The decomposition of H2O2 follows first-order kinetics. If the rate constant is 7.30
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