# Chapter 16

 The flashcards below were created by user mse263 on FreezingBlue Flashcards. general formula for units of k (rate constant) units = (L/mol)order - 1 /unit of time rate expression -1/a x Δ[A]/Δtime = same for b but for c/d 1/c x Δ[C]/Δtime (no negative sign rate law rate = k[A]x[B]y (the reactants); the exponents x & y are orders you need to average the values of k to get full credit integrated rate law for 1st order rxns - kt = ln[A]t - ln[A](rate constant)(time point)=ln[concentration of A at time point] - ln[intitial concentration of A] OR...- kt = ln ([A]t / [A])ororororororoororor[At] = [A]e-kt second order reaction half life DOES depend on initial concentration:t1/2 = 1/k[A] initial first order reaction half life k = ln(2)/t1/2 second order reaction (used to find concentration) follows slope of a straight line (y = mx + b)1/[At] = kt + 1/[A] it takes longer for HALF of the _______ concentration to be consumed smaller concentration; because a smaller concentrsation means there is a smaller quantity of solute meaning it took longer to be consumed because the reaction ran more slowly return to make a flashcard of page 41 in the notes collision theory matter is composed of microscopic particles (molecules/atoms/ions) that are constantly moving and sometimes collide and react activation energy the minimum amount of energy that the reactants must have (before collsions) in order for the reaction to take place; for the reaction to take place the two molecules also must be positioned correctly transition state that state at which there is an intermediate structure which is composed of the reactants combined but not yet separated; represented by the peak on a potential energy profile; the activated complex is present here activated complex the species that exists when reactants are combined but not yet separated; can be found at the peak on a potential energy profile arrhenius equation k = Ae-Ea/RT molecularity the number of reactant molecules shown in each elementary equation; ex: A --> products = unimolecularA + B --> products = bimolecularA + C + D --> products = termolecular catalyst a substance that increases the rate of a chemical reaction without itself undergoing a permanent chemical change in the process; can be identified by observing that whatever about is added or consumed at the beginning of a reaction, the same amount will be produced or remain at the end Authormse263 ID94952 Card SetChapter 16 DescriptionGen Chem II Updated2011-07-27T19:01:08Z Show Answers