CHEM 104 1st Edition Lecture 15Overview of rate laws/integrated rate laws for different order of reactions: Order Rate Law Integrated Rate Law Slope 0 Rate = k [A]t = -kt + [A]0-k1 Rate = k[A] Ln[A]t = -kt +ln[A]0-k2 Rate = k[A]21/[A]t = kt + 1/[A]0kHalf life (t1/2) = the time required for the reactant concentration to drop to half of the initial value - For 1st order reaction: at time t = t1/2, [A]t = [A]0/2T1/2 = ln2/k = 0.693/k1st order half life doesn’t depend on concentration - The half life of a half life is half of the first amount continually decreases by ½ with each half lifeShelf life = the time required for 10% of the reactant to decompose (i.e. 90% remains) - Example: expiration date of pharmaceutical drugs is guarantee date that at least 90% of the drugremainsNanoscale view of reactions- For a reaction to happen, the molecules of the reactant must satisfy the following conditions: o Molecules must have enough energyo Molecules must collideThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- 2 types of elementary reactions: (elementary = simple reactions form which more complex reactions can be build) o Unimolecular (A products): 1 molecule of reactanto Bimolecular (A + B products): 2 molecules of reactants (but A and B can be the same molecule) - Molecularity – how many molecules are involved - Example: cis-2butene trans-2butene is a unimolecular
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