# Chem202 Chap 14 & 15

 .remove_background_ad { border: 1px solid #555555; padding: .75em; margin: .75em; background-color: #e7e7e7; } .rmbg_image { max-height: 80px; } Average reaction rate for A----->B rate=-^A/^trate=^B/^t^ is delta Stoichiometry and Reaction Rate aA+bB---->cC+dD rate=-1/a(^[A]/^t)rate=-1/b(^[B]/^t)rate=1/c(^[C]/^t)rate=1/d(^[D]/^t) rate law aA+bB---->cC+dD rate=k[A]x[B]y reation order and units of k 0====M/s 1====1/s 2====1/Ms 3====1/M2s 1st order half life t1/2=.693/k half life of a first order reaction is independent of the initial concentration of the reactant. 2nd order half life t1/2=1/k[A]o half life is inversely proportional to initial reactant concentration. 0 order half life t1/2=[A]o/2k ? collision theory the reaction rate is directly proportional to the number of molecular collisions per second. ratea=number of collisions/s activation energy Ea minimum amount of energy required to initiate a chemical reaction. activated complex or transition state. when molecules collide in an effective collision. highest amount of potential energy. unimolecular elementary reaction one reactant moleculesA------>products bimolecular elementary reaction two reactant moleculesA+A---->productsA+2B---->products termolecular elementary reaction three reactant moleculesA+B+C--->products reaction order for each reactant in an elementary reaction is equal to its stoichiometric coefficient in the chemical equation for that step. A+A---->products2A------>productsrate=k[A]2 catalyst is a substance that increases the rate of a chemical reaction without itself being consumed. heterogeneoues catalyst the reactant and the catalyst are in different phases. The catalyst is usually a solid and the reactants are either gases or liquids homogenous catalyst the reactants and the catalyst are dispersed in a single phase usually liquid Reversible process A chemical reaction in which the products can also be consumed to produce reactants, a process known as the revers reaction Equilibrium the condition where the forward and reverse reactions are occurring at the same rate and there is no net change in the reactant and products concentrations over time Reaction Quotient (Qc) Qc=[C]c[D]d/[A]a[B]b (also Kc at equilibrium) is the product of the product concentrations over the product of the reactant concentrations with each concentration raised to a power equal to the corresponding stoichiometric coefficients in the balanced chemical equation. Law of Mass Action Equation reversed = 1/Kc1 Equation mulitplied by 2 =(Kc1)2 Two equations added = Kc1*Kc2 Kp=Kc(RT)^n Delta n=number of moles of product-number of moles of reactant Kc=prod/react raised to the power of the coefficient in front if QcKc ---Products to reactants +prod shift left-prod shitf right+react shift right-react shift left + pressure-----shift equil to side w/ fewest moles +volume-----shift equil to side w/ most moles temp is the only factor that changes the equilibrium constant catalyst shifts neither the equilibrium or equilibrium constant .remove_background_ad { border: 1px solid #555555; padding: .75em; margin: .75em; background-color: #e7e7e7; } .rmbg_image { max-height: 80px; } AuthorJamess0688 ID69393 Card SetChem202 Chap 14 & 15 Descriptionfor exam 2 Updated2011-02-28T03:04:11Z Show Answers