Textbook Notes (368,789)
Canada (162,165)
York University (12,867)
Chemistry (270)
CHEM 1001 (72)
Chapter 14

Chemistry 1001-Chap 14 notes.docx

5 Pages
136 Views
Unlock Document

Department
Chemistry
Course
CHEM 1001
Professor
Michael Mozurkewich
Semester
Winter

Description
Chemistry 1001 Chapter 14 – Textbook Notes The Rate of a Chemical Reaction  When one Sn ion is produced for every 2 Fe ions in a chemical reaction, the buildup of Sn will be only the ½ that of Fe ion.  Units for rates: mol/L*s  Increasing concentration, increases the amount of particles colliding  Increasing pressure, increases the action of particles  Increasing temperature, increases the kinetic energy of particles to collide more often  ^ All of them increase the rate of a chemical reaction Measuring Reaction Rates  Initial Rate of a Reaction: is the rate measured over a short time interval at the start of a reaction  Instantaneous Rate of a Reaction: rate measured at any point in reaction often through the slope of a tangent line to a graph of concentration vs. time  Average Rate: rate measured over longer time intervals The Rate Law  It is the relationship between the rate of a reaction and the concentrations of the reactants  Rate of reaction = k [A] [B] n  If m=1, reaction is first order  If n=2, reaction is second order  K is the rate constant: which relates the rate of reaction to reactant concentrations  The larger the value of k, the faster a reaction goes  All unimolecular reactions are first order but not all first order reactions are unimolecular  Al bimolecular reactions are second order but not all second order reactions are bimolecular  Differential Rate Law: Reaction rate as a function of concentration - Gives you rate of reaction at specific concentrations  Integrated Rate Law: Concentration as a function of time - Gives you the amount of time it takes to get from initial concentration of reactant to some other concentration Zero-Order Reactions  Rate of reaction = k [A] = k = constant  Integrated Rate Law: expresses the concentration of a reactant as a function of time  A plot of concentration as a function of time for the zero-order reaction Aproducts, is a straight line with a slope of –k First-Order Reactions  Half-life: is the time required for ½ of a reactant to be consumed  A graph for a first order reaction, it is a straight line with a slope of –k  Half-life is constant Second-Order Reactions  A graph for this would be a straight line with a slope of k  Half-life is not constant – each half life is twice as long as the one preceding it SUMMARY OF BASIC IDEAS OF REACTION KINETICS: PAGE 621 (TABLE) Theoretical Models for Chemical Kinetics  The activation energy: is the minimum kinetic energy that molecules must bring to their collisions for a chemical reaction to occur  The higher the activation energy of a reaction, the smaller is the fraction of energetic collisions and the slower the reaction  Transition state (activated complex): formed through collisions, either dissociates back into the original reactants or forms product molecules  A reaction profile: traces the progress of a reaction, highlighting the energy states of the reactants, the products and the activated complex - Potential energies are plotted on the vertical/horizontal axis against the quantity called “Progress of Reaction” - Delta H: Enthalpy change – difference between reactants and products - The dif
More Less

Related notes for CHEM 1001

Log In


OR

Join OneClass

Access over 10 million pages of study
documents for 1.3 million courses.

Sign up

Join to view


OR

By registering, I agree to the Terms and Privacy Policies
Already have an account?
Just a few more details

So we can recommend you notes for your school.

Reset Password

Please enter below the email address you registered with and we will send you a link to reset your password.

Add your courses

Get notes from the top students in your class.


Submit