Chemistry. Chemical Kinetics - 2 Session Objectives 1.Methods of determining order of a reaction 2.Theories of chemical kinetics 3.Collision theory 4.Transition.

Slides:



Advertisements
Similar presentations
Chapter 12: Chemical Kinetics
Advertisements

KINETICS.
Chapter 12 Chemical 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.
UNIT 3: Energy Changes and Rates of Reaction
Reaction Rates (Chapter 13)
Chapter 14 Chemical Kinetics In kinetics we study the rate at which a chemical process occurs. Lecture Presentation © 2012 Pearson Education, Inc.
Chapter 13 Chemical Kinetics
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 14 Chemical Kinetics
Chapter 14 Chemical Kinetics
Chapter 12 Chemical Kinetics. Chapter 12 Table of Contents Copyright © Cengage Learning. All rights reserved Reaction Rates 12.2 Rate Laws: An.
Integration of the rate laws gives the integrated rate laws
Chemical Kinetics Chapter 12.
Lecture 18 (Ch 18) HW: Ch 18: 1, 3, 15, 41 Kinetics pt 2: Temperature Dependence of Rate Constants.
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 15 Rates of Reaction.
CHEMICAL KINETICS The branch of chemistry which deals with the rate of chemical reactions and the factors which influence the rate of reaction is called.
Dr. Floyd Beckford Lyon College
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
Chemical Kinetics Chapter 14 Chemical Kinetics. Chemical Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed.
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,
Chapter 15 Chemical Kinetics: The Rate of Chemical Reactions.
Chemical Kinetics CHAPTER 14 Part B
Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Chapter 13.
Equilibrium Rate Constant Integrated Rate Law Activation Energy Reaction Mechanisms Rate Laws.
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:
Kinetics The Study of Rates of Reaction. Rate of a Reaction The speed at which the reactants disappear and the products are formed determines the rate.
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.
BLB 11 th Chapter Will the reaction occur? Ch. 5, How fast will the reaction occur? Ch How far will the reaction proceed? Ch. 15.
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.
From the Arrhenius equation we have: 301. From the Arrhenius equation we have: 302.
By- A.P.S. BHADOURIYA M.Sc.(Lko. Uni.) , B.Ed. NET(UGC-CSIR)
AP CHEMISTRY CHAPTER 12 KINETICS. 2 Chemical Kinetics Thermodynamics tells us if a reaction can occur Kinetics tells us how quickly the reaction occurs.
Chapter 14 – Chemical Kinetics The rate of a chemical reaction is the speed at which products or formed and reactants broken down. There factors that affect.
BLB 11 th Chapter Will the reaction occur? Ch. 5, How fast will the reaction occur? Ch How far will the reaction proceed? Ch. 15.
Activation Energy E a : is the minimum energy that reactants must have to form products. the height of the potential barrier (sometimes called the energy.
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.
Dr. Mihelcic Honors Chemistry1 Chemical Kinetics Rates and Mechanisms of Chemical Reactions.
Chpt 12 - Chemical Kinetics Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW set1: Chpt 12 - pg , # 22, 23, 28 Due Fri.
KINETICS. Studies the rate at which a chemical process occurs. a A + b B c C + d D v = - dc/dt = k [A]x [B]y Besides information about the speed at which.
Chpt 12 - Chemical Kinetics Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW set1: Chpt 12 - pg , # 22, 23, 28 Due Jan.
Chemical Kinetics Chemical Kinetics or Rates of reaction.
Kinetics Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions.
Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.
Kinetics. Reaction Rate  Reaction rate is the rate at which reactants disappear and products appear in a chemical reaction.  This can be expressed as.
Chapter 5 Rates of Chemical Reaction. 5-1 Rates and Mechanisms of Chemical Reactions 5-2 Theories of Reaction Rate 5-3 Reaction Rates and Concentrations.
Chemical Kinetics. Slide 2 of 55 Contents 15-1The Rate of a Chemical Reaction 15-2Measuring Reaction Rates 15-3Effect of Concentration on Reaction Rates:
Chemical Kinetics. Kinetics The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can’t tell how fast. (Spontaneity.
1 REACTION KINETICS Reaction rates Reaction order Reaction mechanisms Collision frequency Energy profile diagrams Arrhenius equation Catalysts.
Chapter 13 Chemical Kinetics CHEMISTRY. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of.
16-1 KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS.
Notes 14-4 Obj. 14.5, The half-life of a first-order reaction is equal to _________, where k is the rate constant. a / k b k c. k /2.
Chemical Kinetics. The branch of Physical chemistry which deals with the rate of reactions is called chemical kinetics. The study of chemical kinetics.
AP CHEMISTRY Chapter 14 Chemical Kinetics Chemical Kinetics Study of how rapidly a reaction will occur. In addition to speed of reaction, kinetics.
Chemical Kinetics Unit 10 – Chapter 12.
Second-Order Processes
BY JHERUDDEN PGT (CHEMISTRY) KV SECL,NOWROZABAD
KINETICS CONTINUED.
Second-Order Processes
Presentation transcript:

Chemistry

Chemical Kinetics - 2

Session Objectives 1.Methods of determining order of a reaction 2.Theories of chemical kinetics 3.Collision theory 4.Transition state theory 5.Temperature dependence of rate constant; Arrhenius equation 6.Catalysis 7.Reaction mechanism

Methods of determining the order of a reaction Integrated method The equation which gives a constant value of k decides the order of reaction Graphical method The data are plotted acc to different integrated rate equations so as to yield a straight line.Slope gives the value of rate constant Initial rate method Concentration of one of the reactant is varied Half life method In this method we plot half life of the reactant versus concentration of the reactant.

Methods of determining the order of a reaction L mole -1 sec -1 k1/[A] vs tSecond sec -1 -kIn[A] vs t[A]=[Ao]e -kt First Mole l -1 sec -1 -k[A] vs t[A]=[Ao]-ktZero Units of rate constant Slope of kineti cs plot Characteristi c kinetics Plot Integrated rate law Differential rate law Reaction Order

Graphical Representation

Conc. [A] t log [A] tt 1/ [A] Graphical representation for concentration of integrated rate equation versus time zero orderfirst ordersecond order Graphical Representation

Illustrative Example For the thermal decomposition of CH 3 CHO; CH 3 CHO = CH 4 (g) + CO(g) The following rate data are obtained. ExperimentInitial pressureInitial rate of increase in total pressure Predict the order of the reaction.

Solution Let the expression for the rate of the reaction is r = k[CH 3 CHO] n Putting the values for both experiments separately Thus, 0.61 = k (300) n 0.27 = k (200) n Dividing both equations and taking log of the resultant equation or n = 2.0

Initial rate method Complications occurs when multiple reactant are involved in the reaction. This method involves the determination of the order of each reactant separately. To determine the order of a particular reactant, its concentration is varied keeping the concentrations of other reactants constant. In every experiment, we determine the initial rate of the reaction and observe the dependence of rate on that particular reactant. Keeping [B] constant

Illustrative Example Rate of the reaction; A + B = products; is given below as a function of the initial concentration of ‘A’ and ‘B’. [A](mol L -1 )[B](mol L -1 )rate(mol L -1 min -1 ) Determine the order of the reaction with respect to ‘A’ and ‘B’. For first two experiments, the concentration of the reactant ‘B’ is constant. Rate of the reaction depend linearly on reactant ‘A’. Now, taking experiments first and third, the concentration of the reactant ‘A’ is constant. Therefore, rate of the reaction is independent of ‘B’. Thus, order of the reaction with respect to ‘A’ = one. Order of the reaction with respect to ‘B’ = zero. Solution:

Half life method

Illustrative Example The half-life of a particular chemical reaction at two different initial concentrations 5 x and 25 x10 -5 M are 2 and 16 hours. Calculate the order of reaction. Solution:

Integrated method In this method, we put the data into the integrated form of the rate laws and calculate the values of the rate constants for different kinetics of the reaction. The order of the reaction is that one for which the value of rate constant is constant.

Some first order reactions Decomposition of H 2 O 2 Let V o & V t be volume of KMnO 4 used during zero & time t respectively

Some first order reactions Hydrolysis of ester Let V 0, V t be the volume of alkali required for titration during 0,t & infinite time

Theories of chemical kinetics 1. Collision theory 2. Transition state theory

Collision theory Reaction occurs when reacting species have sufficient energy to collide and proper orientation in space. Energy barrier: The minimum energy which the colliding particles possess in order to bring about the chemical reaction is called threshold energy(activation energy). Orientation barrier: Colliding molecules should be in their proper orientation at the time of collision.

Transition State Theory In the activated complex theory, we consider two reactants approaching and their potential energy rising and reaching a maximum. Activation energy - the energy needed to start a chemical reaction. It is very low for some reactions and very high for others.

Some Points about E a 1. E a is always positive. 2. The larger the value of E a, the slower the rate of a reaction at a given temperature. 3. The larger the value of E a, the steeper the slope of (ln k) vs (1/T). A high activation energy corresponds to a reaction rate that is very sensitive to temperature. 4.The value of E a itself DOES NOT CHANGE with temperature.

Effect of temperature on rate of chemical reaction The ratio is called the temperature coefficient and its value is 2 or 3 A is frequency factor or Arhenius constant,E a is activation energy Plot of log k vs 1/T is a straight line & slope =-E a /2.303R

Temperature Dependence Plot of log k vs 1/T is a straight line & slope =-E a /2.303R

Illustrative Example If we plot log k versus 1/T,we get a straight line. What is the slope and intercept of the line. intercept = log k. Taking log of both sides Solution:

Effect of temperature on rate of chemical reaction

Illustrative Example The activation energy of one of the reactions in the Krebs citric acid cycle is 87 kJ/mol. What is the change in the rate constant when the temperature falls from 37 o C to 15 o C? Solution:

= cals E a = K cals The specific reaction rate for a reaction increases by a factor 4 if the temperature is changed from 27 o C to 47 o C. Find the activation energy for the reaction. Illustrative Example Solution:

Catalysis Catalyst: A substance that changes the rate of a reaction without being consumed in the reaction. Provides an easier way to react. Lower activation energy. Still make the same products. Enzymes are biological catalysts. Inhibitor: A substance that decreases the rate of reaction (a negative catalyst).

How catalyst change reaction rate Catalysts are the one way to lower the energy of activation for a particular reaction. The presence of the catalyst alters the path of the reaction. The lower activation energy allows the reaction to proceed faster.

Rate Law and Mechanism A mechanism is a collection of elementary steps devised to explain the reaction in view of the observed rate law. For the reaction, 2 NO 2 (g) + F 2 (g)  2 NO 2 F (g), the rate law is, rate = k [NO 2 ] [F 2 ]. Can the elementary reaction be the same as the overall reaction? If they were the same the rate law would have been rate = k [NO 2 ] 2 [F 2 ], Therefore, the overall reaction is not an elementary reaction.

Rate-determining Step in a Mechanism Slowest step: The rate determining step is the slowest elementary step in a mechanism, and the rate law for this step is the rate law for the overall reaction. Steady-state approximation: The steady-state approximation is a general method for deriving rate laws when the relative speed cannot be identified. It is based on the assumption that the concentration of the intermediate is constant.

Illustrative Problem The hypothetical reaction follows the following mechanism The order of the overall reaction is (a) 0(b) 1 (c) 2(d) 3/2

Solution The order depends on slowest step Hence, the answer is (d).

Illustrative Problem The decomposition of ozone is believed to occur by mechanism O 3 O 2 + O (fast), O + O 3 2O 2 (slow) When the concentration of O 2 is increased, the rate (a) increases(b) decreases (c) remains the same(d) Cannot say

Solution  When concentration of O 2 is increased rate decreases.

Illustrative Example The decomposition of H 2 O 2 in the presence of I – follow this mechanism, i H 2 O 2 + I –  H 2 O + IO – (k 1 )slow ii H 2 O 2 + IO –  H 2 O + O 2 + I – (k 2 )fast What is the rate law? The slow step determines the rate, and the rate law is: rate = k1 [H 2 O 2 ] [I – ] Since both [H 2 O 2 ] and [I – ] are measurable in the system, this is the rate law. Solution

Illustrative Example The (determined) rate law is, rate = k [NO 2 ] [F 2 ], for the reaction, 2 NO 2 (g) + F 2 (g)  2 NO 2 F (g), and a two-step mechanism is proposed: i NO 2 (g) + F 2 (g)  NO 2 F (g) + F (g) ii NO 2 (g) + F (g)  NO 2 F (g) Which is the rate determining step? The rate for step i is rate = k [NO 2 ] [F 2 ], which is the rate law, this suggests that step i is the rate- determining or the slow step. Solution:

Illustrative Problem At 380° C, the half-life period for the first order decomposition of H 2 O 2 is 360 min. The energy of activation of the reaction is 200 kJ mole -1. Calculate the time required for 75% decomposition at 450° C.

Solution

Thank you