Integrated Rate Law.

Slides:

Advertisements

Similar presentations

KINETICS -REACTION RATES

Advertisements

Kinetics ; 13.11; December Assigned HW 13.22, 13.24, 13.26, 13.34, 13.36, 13.58, Due: Monday 6-Dec Lecture 33 1.

Chpt 12 - Chemical Kinetics Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW: Chpt 12 - pg , #s Due Fri Jan. 8.

Elementary Chemical Kinetics ( )

Example 5:Example 5:  Determine the rate law for the following reaction----  NH 4 + (aq) + NO 2 - (aq)  N 2(g) + 2H 2 O (l) Experiment[NH 4 + ] initial.

Chapter 13 Integrated Rate Laws I.Integrated Rate Laws A.Preview: So far, we have looked at rate as a function of concentration Next, we look at concentration.

Slide 1 of Zero-Order Reactions A → products R rxn = k [A] 0 R rxn = k [k] = mol L -1 s -1.

© University of South Carolina Board of Trustees 1 st -Order Rate Law Differential Form Rate = k [A]( t ) Integral Forms [A]( t ) = [A] 0 e - kt ln [A](

Chemical Kinetics Chapter 14. The Rate Law Rate law – description of the effect of concentration on rate aA + bB cC + dD Rate = k [A] x [B] y reaction.

Every slope is a derivative. Velocity = slope of the tangent line to a position vs. time graph Acceleration = slope of the velocity vs. time graph How.

Chemical Kinetics © 2009, Prentice-Hall, Inc. First-Order Processes Therefore, if a reaction is first-order, a plot of ln [A] vs. t will yield a straight.

Integrated Rate Laws. Quick Review Our previous lessons have focused on calculating the rate of a reaction and rate constant by observing how changes.

The rate of reaction.

Speed vs. Time Graphs.

Chemical Kinetics The area of chemistry that concerns reaction rates and reaction mechanisms.

11.2 Reaction Rate and Concentration

Kinetics. This is important!!! determine rate laws & units from experimental data calculate rates & concentrations of reactants or products under given.

What is this?. Kinetics Reaction Rates: How fast reactions occur.

Integrated Rate Law. Rate laws can be converted into equations that tell us what the concentration of the reactants or products are at any time Calculus.

Rate Law & Reaction Order 02

Kinetics Until now, we have considered that reactions occur: Reactants form products and conservation of mass is used to find amounts of these Now, we.

Integrated Rate Laws 02/13/13

Chapter 14 Chemical Kinetics Chemical Kinetics CH 141.

Integrated Rate Laws How to solve.

Measuring Reaction Rates Continuous monitoring polarimetry spectrophotometry total pressure Taking aliquots gas chromatography titration for one of the.

Integrated Rate Law Goal: To determine the order and rate law from concentration and time data.

Second and Zero rate orders Chapter 14 part IV. Second Order Rate Laws  Butadiene forms its dimer  2C 4 H 6 (g) - > C 8 H 12 (g)

Rate Law and Activation Energy Methyl Blue Determining the Rate Law using the Time Dependent Rate.

 Rate laws can be converted into equations that tell us what the concentration of the reactants or products are at any time  Calculus required to derive.

Expresses the reactant concentrations as a function of time. aA → products Kinetics are first order in [A], and the rate law is Rate = k[A] Integrated.

AP Chem Kinetics integrated rate laws, half life.

Reaction Rates Measures concentration (molarity!) change over time Measures concentration (molarity!) change over time Example: Example: 2H 2 O 2  2H.

From Method of Initial Rates to Integrated Rate Law

Types of Rate Laws First Order Second Order Zero Order.

1. For the reaction A + B  C, the rate constant at 215 o C is 5.0 x /s and the rate constant at 452 o C is 1.2 x /s. What is the activation.

Ch 14- Chemical Kinetics -The area of chemistry concerned with the speeds, or rates, of reactions.

Pre-Lab Rate Law Determination of the Crystal Violet Reaction

Rate Laws Example: Determine the rate law for the following reaction given the data below. H2O2 (aq) + 3 I- (aq) + 2H+ (aq) I3- (aq) + H2O (l) [H2O2]

#39 A first-order reaction is 38. 5% complete in 480. s. a

14.4 Change of rate with time

Introduction to Reaction Rates

Integrated Rate Law.

The Changes of Concentration with Time

Rates and Rate Laws.

Reaction rate and rate laws

Zero, First & Second Rate orders

Integrated Rate Law Expresses the reactant concentrations as a function of time. aA → products Kinetics are first order in [A], and the rate law is Rate.

AP Chem Work on warm up problem Important Dates:

First-Order Rate = k[A] Integrated: ln[A] = –kt + ln[A]o

Rates and Rate Laws.

A graphing calculator is required for some problems or parts of problems 2000.

Kinetics sample problems

Introduction to Reaction Rates

Integrated Rate Law: First-Order

Integrated Rate Law.

Rates and Rate Laws.

Review Differential Rate Laws ... rate (M s-1) = k [A]a [B]b

Chapter 12 Chemical Kinetics.

Chapter 16 Chemical Kinetics.

Review Differential Rate Laws ... rate (M s-1) = k [A]a [B]b

Review Differential Rate Laws ... rate (M s-1) = k [A]a [B]b

Review Differential Rate Laws ... rate (M s-1) = k [A]a [B]b

Reaction Rates Popcorn Activity.

Objectives: What does reaction order mean?

Integrated Rate Law By Chloe Dixon

Review Differential Rate Laws ... rate (M s-1) = k [A]a [B]b

Integrated Rate Laws Describe how the concentration of reactants changes over TIME Compare this to the Differential Rate laws that describe how the concentration.

Presentation transcript:

Integrated Rate Law

Integrated Rate Law This law is used when you are given __________ & __________ Yesterday (for the differential rate law) you were given a graph of concentration & rate

Rate Law Summary

Determining the order: You will be given a chart of concentrations and time Make another column for __________ and __________ Use a few data points to find the slope of [A] vs time Do the same for ln[A] vs time Do the same for 1/[A] vs time The one that gives the straightest line gives the reaction order

Example Determine the rate law & the value of k for the following reaction: 2N2O5  4NO2 + O2 [N2O5] Time (s) 0.0707 50 0.0500 100 0.0250 200 0.0125 300 0.00625 400

½ life Time it takes for ½ the reactant to be gone What was the ½ life for the last problem?

Example Determine the rate law & the value of k for the following reaction: 2C4H6  C8H12 [C4H6] Time (s) 0.01 0.00625 1000 0.00467 1800 0.00370 2800 0.00313 3600 0.00270 4400 0.00241 5200 0.00208 6200

Example What is the ½ life for the last reaction?

Another example A 1st order reaction is 38.5% complete in 480 seconds Calculate the rate constant Calculate the value of the ½ life How long will it take for the reaction to go 25% 75% 95%

Last example If the ½ life is 45 seconds, how much is left after 225 seconds?