Cmc chapter 16

Chapter Menu Reaction Rates Section 16.1 A Model for Reaction Rates Section 16.2 Factors Affecting Reaction Rates Section 16.3 Reaction Rate Laws Section 16.4 Instantaneous Reaction Rates and Reaction Mechanisms Exit Click a hyperlink or folder tab to view the corresponding slides.

Section 16-1 Section 16.1 A Model for Reaction Rates ,[object Object],energy: the ability to do work or produce heat; it exists in two basic forms: potential energy and kinetic energy ,[object Object]

Section 16-1 Section 16.1 A Model for Reaction Rates (cont.) reaction rate collision theory activated complex activation energy Collision theory is the key to understanding why some reactions are faster than others.

Section 16-1 Expressing Reaction Rates ,[object Object]

Section 16-1 Expressing Reaction Rates (cont.) ,[object Object]

Section 16-1 Collision Theory ,[object Object]

Section 16-1 Collision Theory (cont.) ,[object Object]

Section 16-1 Collision Theory (cont.) ,[object Object],[object Object]

Section 16-1 Collision Theory (cont.)

Section 16-1 Spontaneity and Reaction Rate ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 16-1 Section 16.1 Assessment Which of the following is NOT a requirement for a reaction to occur, according to the collision theory? A. Reacting substances must collide. B. Reacting substances must be in an exothermic reaction. C. Reacting substances must collide in the correct orientation. D. Reacting substances must collide with sufficient energy to form an activated complex.

[object Object],[object Object],[object Object],[object Object],Section 16-1 Section 16.1 Assessment A temporary, unstable arrangement of atoms in which old bonds are breaking and new bonds are forming is called ____. A. reaction complex B. reaction substrate C. activated complex D. activated molecule

Section 16-2 Section 16.2 Factors Affecting Reaction Rates ,[object Object],concentration: a quantitative measure of the amount of solute in a given amount of solvent or solution catalyst inhibitor heterogeneous catalyst homogeneous catalyst ,[object Object],Factors such as reactivity, concentration, temperature, surface area, and catalysts affect the rate of a chemical reaction.

Section 16-2 The Nature of Reactants ,[object Object]

Section 16-2 Concentration ,[object Object],[object Object]

Section 16-2 Surface Area ,[object Object],[object Object],[object Object]

Section 16-2 Temperature ,[object Object],[object Object],[object Object]

Section 16-2 Temperature (cont.) ,[object Object],[object Object]

Section 16-2 Temperature (cont.)

Section 16-2 Catalysts and Inhibitors ,[object Object],[object Object]

Section 16-2 Catalysts and Inhibitors (cont.) ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 16-2 Section 16.2 Assessment Which of the following generally does not increase the rate of a chemical reaction? A. increasing concentration B. adding a catalyst C. adding an inhibitor D. increasing temperature

[object Object],[object Object],[object Object],[object Object],Section 16-2 Section 16.2 Assessment High-energy particle collisions are more frequent: A. when an inhibitor is present B. when temperature is decreased C. when activation energy is higher D. when temperature is increased

Section 16-3 Section 16.3 Reaction Rate Laws ,[object Object],reactant: the starting substance in a chemical reaction rate law specific rate constant reaction order method of initial rates ,[object Object],The reaction rate law is an experimentally determined mathematical relationship that relates the speed of a reaction to the concentrations of the reactants.

Section 16-3 Writing Reaction Rate Laws ,[object Object],[object Object]

Section 16-3 Writing Reaction Rate Laws (cont.) ,[object Object],[object Object]

Section 16-3 Writing Reaction Rate Laws (cont.) ,[object Object],[object Object],[object Object]

Section 16-3 Writing Reaction Rate Laws (cont.) ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Section 16-3 Determining Reaction Order ,[object Object],[object Object]

Section 16-3 Determining Reaction Order (cont.)

Section 16-3 Determining Reaction Order (cont.) ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 16-3 Section 16.3 Assessment What is the overall reaction order of the following reaction? Rate = k [A] 2 [B] 2 A. 1st B. 2nd C. 3rd D. 4th

[object Object],[object Object],[object Object],[object Object],Section 16-3 Section 16.3 Assessment In the following reaction, what is the overall reaction order if doubling [A] results in quadrupling the reaction rate and doubling [B] results in a reaction rate eight times faster? Rate = k [A] m [B] n A. 12 B. 5 C. 6 D. 10

Section 16-4 Section 16.4 Instantaneous Reaction Rates and Reaction Mechanisms ,[object Object],decomposition reaction: a chemical reaction that occurs when a single compound breaks down into two or more elements or new compounds ,[object Object],[object Object]

Section 16-4 Section 16.4 Instantaneous Reaction Rates and Reaction Mechanisms (cont.) instantaneous rate complex reaction reaction mechanism intermediate rate-determining step The slowest step in a sequence of steps determines the rate of the overall chemical reaction.

Section 16-4 Instantaneous Reaction Rates ,[object Object],[object Object]

Section 16-4 Instantaneous Reaction Rates (cont.) ,[object Object],[object Object],[object Object],[object Object],[object Object]

Section 16-4 Reaction Mechanisms ,[object Object],[object Object],[object Object]

Section 16-4 Reaction Mechanisms (cont.) ,[object Object],[object Object],[object Object]

Section 16-4 Reaction Mechanisms (cont.)

Section 16-4 Reaction Mechanisms (cont.) ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 16-4 Section 16.4 Assessment What is a reaction with two or more elementary steps called? A. compound reaction B. complex reaction C. multi-step reaction D. combined reaction

[object Object],[object Object],[object Object],[object Object],Section 16-4 Section 16.4 Assessment What is the slowest step in a complex reaction called? A. elementary step B. reducing step C. rate-determining step D. intermediate step

Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

Study Guide 1 Section 16.1 A Model for Reaction Rates Key Concepts ,[object Object],[object Object],[object Object],[object Object]

Study Guide 2 Section 16.2 Factors Affecting Reaction Rates Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 3 Section 16.3 Reaction Rate Laws Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 4 Section 16.4 Instantaneous Reaction Rates and Reaction Mechanisms Key Concepts ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 1 The energy required to initiate a reaction is called ____. A. initiation energy B. activation energy C. complex energy D. catalyst energy

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 2 In general, which of the following does not cause a reaction rate to increase? A. increasing surface area B. increasing temperature C. increasing volume D. adding a catalyst

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 3 What is the overall reaction order of the following reaction? Rate = k [A][B] 2 [C] A. 1st order B. 2nd order C. 3rd order D. 4th order

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 4 A substance produced by an elementary step in a complex reaction that is consumed later and does not show up in the net reaction is called a(n) ____. A. activated complex B. catalyst C. enzyme D. intermediate

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 5 Increasing the temperature of a reaction increases the rate of reaction by: A. increasing the collision frequency B. increasing the number of high-energy collisions C. both a and b D. none of the above

[object Object],[object Object],[object Object],[object Object],STP 1 Which of the following is an acceptable unit for expressing a rate? A. mol/L ● s B. L/s C. M D. mL/h

[object Object],[object Object],[object Object],[object Object],STP 2 How many moles are in 4.03 × 10 2 g of calcium phosphate (Ca 3 (PO 4 ) 2 )? A. 0.721 moles B. 1.39 moles C. 1.54 moles D. 3.18 moles

[object Object],[object Object],[object Object],[object Object],STP 3 Doubling the concentration of one reactant in a reaction causes the reaction rate to double. What is the order of that reactant? A. 1st B. 2nd C. unable to determine D. none of the above

[object Object],[object Object],[object Object],[object Object],STP 4 The rate law for the reaction A + B + C -> Product is rate = k [A] 2 [B][C]. If [A] = 0.350M, [B] = .500M, [C] = .125M, and k = 6.50 × 10 –5 L 3 /(mol 3 ● s), what is the instantaneous rate of reaction? A. 2.84 × 10 –6 mol/L ● s B. 4.98 × 10 –7 mol/L ● s C. 5.84 × 10 –6 mol/L ● s D. 2.84 × 10 –7 mol/L ● s

[object Object],[object Object],[object Object],[object Object],STP 5 H 2 O 2 breaks down to form hydrogen and oxygen gas in what type of reaction? A. synthesis B. double replacement C. decomposition D. single replacement

IB Menu Click on an image to enlarge.

CIM Figure 16.4 Effect of Molecular Orientation on Collision Effectiveness

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Cmc chapter 16

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Cmc chapter 16