A.P. Exam Review Regular Review Day 4. Big Idea #4 Rates of chemical reactions are determined by details of the molecular collisions.

Slides:



Advertisements
Similar presentations
Chemical Kinetics Reaction rate - the change in concentration of reactant or product per unit time.
Advertisements

Reaction Rates What affects the rate of reaction?.
Collision Theory For a rx to occur reacting molecules must collide so 1 - The old bonds “loosen up”, or start to break apart 2 - The correct orientation.
CHEMICAL KINETICS CHAPTER 17, Kinetics Fall 2009, CHEM
Kinetics Quick Review. Radioactive Decay and Kinetics.
AP Chapter 14.  Chemical kinetics is the area of chemistry that involves the rates or speeds of chemical reactions.  The more collisions there are between.
Nanochemistry NAN 601 Dr. Marinella Sandros Lecture 5: Kinetics
Chapter 16: Kinetics Rates and Mechanisms of Chemical Reactions 16.1 Factors That Influence Reaction Rate 16.2 Expressing the Reaction Rate 16.3 The Rate.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.
CHE MODULE 3 CHAPTER 15 LECTURE NOTES. Chemical Kinetics  Chemical kinetics - study of the rates of chemical reactions and is dependent on the.
Reaction Rate Change in concentration of a reactant or product per unit time. [A] means concentration of A in mol/L; A is the reactant or product being.
Chapter 12 Chemical Kinetics. Chapter 12 Table of Contents Copyright © Cengage Learning. All rights reserved Reaction Rates 12.2 Rate Laws: An.
Chapter 15 Kinetics. Kinetics Deals with the rate of chemical reactions Deals with the rate of chemical reactions Reaction mechanism – steps that a reaction.
Chemical Kinetics Rates of chemical reaction - definition of reaction rate - integrated and differential rate law - determination of rate law Mechanism.
Section 2.8—Speeding Up A Reaction
Chemical Kinetics Collision Theory: How reactions takes place
Chemical Kinetics Chapter 16. Chemical Kinetics Thermodynamics – does a reaction take place? Kinetics – how fast does a reaction proceed? Reaction rate.
Chemical Kinetics: Rates and Mechanisms of Chemical Reactions General Chemistry: An Integrated Approach Hill, Petrucci, 4 th Edition Mark P. Heitz State.
Ch 15 Rates of Chemical Reactions Chemical Kinetics is a study of the rates of chemical reactions. Part 1 macroscopic level what does reaction rate mean?
Chemical Kinetics Chapter 16. Kinetics Reaction Rates Factors affecting rate Quantitative rate expressions DeterminationFactors Models for Rates Reaction.
Chapter 14: Rates of Reaction Chemistry 1062: Principles of Chemistry II Andy Aspaas, Instructor.
Dr. Floyd Beckford Lyon College
Chapter 12 Chemical Kinetics. Chapter 12 Table of Contents Copyright © Cengage Learning. All rights reserved Reaction Rates 12.2 Rate Laws: An.
Chemical Kinetics. Kinetics In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at which reactions occur,
= rate = rate constant derived definition: Rate law can be written from molecularity Lowers the E a by making a new ______________ Why? Experimentally.
Chapter 12 Chemical Kinetics.
Chapter 12 Chemical Kinetics How often does Kinetics appear on the exam? Multiple-choice 4-8% (2-5 Questions) Free-response: Almost every year Kinetics:
Chemical Kinetics Chapter 12. Chemical Kinetics The area of chemistry that concerns reaction rates.
1 Chemical Kinetics The area of chemistry that concerns reaction rates. The area of chemistry that concerns reaction rates.
Reaction Rate Change in concentration of a reactant or product per unit time. [A] means concentration of A in mol/L; A is the reactant or product being.
Chemical Kinetics Two Types of Rate Laws 1.Differential- Data table contains RATE AND CONCENTRATION DATA. Uses “table logic” or algebra to find the order.
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
1 Reaction Mechanism The series of steps by which a chemical reaction occurs. A chemical equation does not tell us how reactants become products - it is.
Chemical Kinetics. Kinetics The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can’t tell how fast. (Spontaneity.
AP CHEMISTRY CHAPTER 12 KINETICS. 2 Chemical Kinetics Thermodynamics tells us if a reaction can occur Kinetics tells us how quickly the reaction occurs.
TOPIC D: ARRHENIUS EQUATION AND CATALYSTS. Arrhenius Said the reaction rate should increase with temperature. At high temperature more molecules have.
Chapter 121 Chapter 12: Kinetics; Outline 1. Introduction  2. macroscopic determination of rate (experimental) define rate  define rate law, rate constant,
Kinetics How fast does your reaction go?. Reaction rates Rate is how fast a process occurs Rates are measured in units of Results Time Example: speed.
Reaction Mechanisms Overall Reaction: A → Z
Kinetics Chapter 12. Reaction Rates  Kinetics is concerned with studying the reaction mechanism of a reaction.  An average reaction rate describes how.
A Radioactivity Example Carbon-14 is unstable. It decays very slowly by a process called beta-decay. A beta particle is an electron. It is ejected from.
Kinetics Chemistry—Introduction
Chemical Kinetics By: Ms. Buroker. Chemical Kinetics Spontaneity is important in determining if a reaction occurs- but it doesn’t tell us much about the.
Chpt 12 - Chemical Kinetics Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW set1: Chpt 12 - pg , # 22, 23, 28 Due Fri.
CHEMICAL KINETICS H 2 S (g) + Zn 2+ (aq) ⇆ ZnS (s) + 2H + (aq) Chemical reactions can be viewed from different perspectives 4D-1 (of 21) STOICHIOMETRY.
Chpt 12 - Chemical Kinetics Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW set1: Chpt 12 - pg , # 22, 23, 28 Due Jan.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Kinetics The area of chemistry that concerns reaction rates.
Prepared by PhD Halina Falfushynska. C(s, diamond) C(s, graphite) ΔH ° rxn = Is the reaction favorable?
Reaction Rates: 2 NO2  2 NO + O2 change in conc. 1. slope =
Chemical Kinetics The speed with which chemical reactions occur depends on external conditions The area of chemistry concerned with the speed at which.
CHEM 1212 Exam 2 Review Presented by UGA’s Academic Resource Center 02/28/16.
Kinetics Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions.
Kinetics. Reaction Rate  Reaction rate is the rate at which reactants disappear and products appear in a chemical reaction.  This can be expressed as.
AP CHEMISTRY Chapter 14 Chemical Kinetics Chemical Kinetics Study of how rapidly a reaction will occur. In addition to speed of reaction, kinetics.
Reaction Process. A reaction mechanism is a step by step sequence of reactions that show an overall chemical change The same reaction can occur by different.
Chemical Kinetics Unit 10 – Chapter 12.
Reactions rate and Collision Theory
Introduction to Reaction Rates
Reaction Process.
Kinetics By: Anderson Clark.
Chemical Kinetics Chapter 12.
Kinetics and Rate Law.
Chemical Kinetics.
Reaction Rates: 2 NO2  2 NO + O2 change in conc. 1. slope =
Kinetics.
Introduction to Reaction Rates
Chapter 12 Chemical Kinetics
Chemical Kinetics Chapter 13.
Rate Affecting Factors
Unit 4: Kinetics Collision Theory.
Presentation transcript:

A.P. Exam Review Regular Review Day 4

Big Idea #4 Rates of chemical reactions are determined by details of the molecular collisions.

Enduring Understanding A Reaction rates that depend on temperature and other environmental factors are determined by measuring changes in concentrations of reactants or products over time.

Enduring Understanding B Elementary reactions are mediated by collisions between molecules. Only collisions having sufficient energy and proper relative orientation of reactants lead to products.

Enduring Understanding C Many reactions proceed via a series of elementary reactions.

Enduring Understanding D Reaction rates may be increased by the presence of a catalyst.

= rate = rate constant derived definition: Rate law can be written from molecularity Lowers the E a by making a new ______________ Why? Experimentally derived rate laws show that all reactions aren’t elementary k = zpe -E a /RT k = ln k= Relating [ ] vs. time 1st order: 2nd order: 0 order: Ch. 12 A.P. Chem. Chemical Kinetics Reaction RatesMechanisms -  [ ]  time Avg. Rates Instantaneous Rates Slope of the line tangent at that moment Rate Law k [ ] x experimentally Method of initial rates Constant rates [ ]’s for certain substances high Zero order in one substance Compare runs with all but one [ ] constant Integrated Rate Laws ln[ ] = -kt + ln[ ] 0 1/[ ] = kt + 1/[ ] 0 [ ] = -kt +[ ] 0 ln([ ]/[ ] 0 ) = -kt 0.693/k 1/k[ ] 0 [ ] 0 /2k t½t½ series of steps by which a reaction occurs Elementary steps Inter- mediates RDS catalysts mechanism: Used in one step, produced in another Produced in one step, used in another with a new and faster (dictates) Speeds up a reaction without being consumed collision theory Effective collisions enough energy Break and make new bonds transitional particle activated complex...seen on P.E. diagram Proper orientation Ae -E a /RT (-E a /R)1/T + lnA Arrhenius Equation(s) order

Beta Radiation Electron Capture Alpha Radiation ________