1 Chapter 5 Chemical Reactions 5.8 Energy in Chemical Reactions.

Slides:



Advertisements
Similar presentations
Reaction Rates What affects the rate of reaction?.
Advertisements

Tro IC3 1.Increasing temperature 2.Decreasing temperature 3.Increasing reactant concentration 4.Increasing the surface area of a solid reactant 5.All of.
Collision Theory and Reaction Rate. a) Collision Theory: THE HOME RUN ANALOGY: In order to hit a home run out of the park) one must: ________________________.
Reaction Rates, Catalysts and Collision Theory. Rates of reaction The rate of a reaction measures how fast it happens. Increased reaction rate means that.
Who Wants To Be A Millionaire?
Chemical Reactions Factors Affecting Rates of Reaction January 9, 2015.
Reaction Rates Collision Theory  In order for reactions to occur, particles must collide  If collisions are too gentle, no reaction occurs  If collisions.
© 2013 Pearson Education, Inc. Chapter 9, Section 1 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 9 © 2013 Pearson.
Collision Theory of Reactions A chemical reaction occurs when: Collisions between molecules have sufficient energy to break the bonds in the reactants.Collisions.
Homework Read pages: Answer questions from packet on pages:
Unit 7: Reaction Energy SECTION 1: REACTION RATE.
Section 1Chemical Reactions 〉 When do chemical reactions take place? 〉 Chemical reactions occur when substances undergo chemical changes to form new substances.
KEY CONCEPT Life depends on chemical reactions.
General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc. 1 Chapter 9 Chemical Equilibrium 9.5 Changing Equilibrium Conditions:
1 What is a physical change? In a physical change, identity and composition substance do not change. state can change or material can be torn into smaller.
General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc. 1 Collision Theory of Reactions A chemical reaction occurs when  collisions.
Copyright © 2004 Pearson Education Inc., publishing as Benjamin Cummings. 1 Chapter 6 Chemical Reactions 6.5 Oxidation-Reduction Reactions.
Chapter 16 Equilibrium. How do chemical reactions occur? Collision Model Molecules react by colliding into one another. – This explains why reactions.
Chemical Reactions and Enzymes Chapter 2-4. Chemical Reactions Chemistry is what life does!!! EVERYTHING that happens in an organism occurs because of.
Chemical Change: Energy, Rate and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy.
Chapter 5 Chemical Quantities and Reactions Chapter 5 Chemical Quantities and Reactions 5.7 Mole Relationships in Chemical Equations 1.
General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 6.9 Energy Changes in Chemical Reactions Chapter 6 Chemical Reactions and Quantities.
Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 9 Chemical Quantities in Reactions 9.5 Energy in Chemical Reactions Cold packs use an.
Exothermic and Endothermic Reactions. - What is Exothermic and Endothermic Reactions ? Exothermic reactions : Reactions accompanied with producing heat.
Chemistry of Life Chapter 2. All Living Things Use Energy Energy in living things is converted from 1 form to another (chemical-physical-thermal etc.)
Kinetics.
© 2013 Pearson Education, Inc. Chapter 9, Section 1 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 9 © 2013 Pearson.
Chemistry An Introduction to General, Organic, and Biological Chemistry, Eleventh Edition Copyright © 2012 by Pearson Education, Inc. Chapter 5 Chemical.
The Nature of Chemical Reactions Chapter 7.1 Notes.
General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc. 1 Chapter 9 Chemical Equilibrium 9.1 Rates of Reactions.
Chapter 12 Chemical Equilibrium Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.
Reaction Theory: Collision, Activation and Potential Energy Diagrams (Chapter 16 Lesson 1&2)
1 Collision Theory Molecules must collide in order to react. Molecules must collide with the proper orientation such that the correct atoms can form a.
1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 6 Lecture Outline Prepared by Andrea D. Leonard.
CHEMICAL EQUILIBRIUM. INTRODUCTION 1. In the reaction: I 2 (g) + H 2 (g)  2 HI(g) at 150 o C, the original color of the mixture is: at 150 o C, the original.
Reactions rate and Collision Theory
Collision Theory of Reactions
Chapter 10 Reaction Rates and Chemical Equilibrium
Chapter 5 Chemical Quantities and Reactions
Reaction Rates.
KEY CONCEPT Life depends on chemical reactions.
2. Classifying based on energy transfer
Trilogy – Chemistry – CHAPTER 5 – Energy changes
KEY CONCEPT Life depends on chemical reactions.
or How Chemical Reactions Occur
Chapter 5 Chemical Quantities and Reactions
KEY CONCEPT Life depends on chemical reactions.
Chemical Reactions.
Chapter 9 Chemical Equilibrium
Chapter 5 Chemical Quantities and Reactions
Rates of Chemical Reactions
KEY CONCEPT Life depends on chemical reactions.
General, Organic, and Biological Chemistry
Chemical Kinetics.
Reaction Rates Chapter 7 Section 4.
and Chemical Equilibrium
ENERGY & CHEMICAL CHANGE
Reaction Rate & Activation Energy
Chapter 7.1 – Nature of Chemical Reactions
EQUILIBRIUM.
Kinetics and Equlibrium
Exothermic & Endothermic
Chapter 13 Reaction Rates and Chemical Equilibrium
Higher Revision Slides
התנאים הנחוצים להתרחשות של תגובה כימית
Chapter 5 Chemical Reactions and Quantities
Unit 8: Rates of Reactions
Section 1: Reaction Rate
Chapter 17 Equilibrium Reversible Reactions.
Chapter 5 Chemical Quantities and Reactions
Presentation transcript:

1 Chapter 5 Chemical Reactions 5.8 Energy in Chemical Reactions

2 Collision Theory of Reactions A chemical reaction occurs when collisions between molecules have sufficient energy to break the bonds in the reactants. bonds between atoms of the reactants (N 2 and O 2 ) are broken and new bonds (NO) can form. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

3 Activation Energy The activation energy is the minimum energy needed for a reaction to take place. When a collision provides energy equal to or greater than the activation energy, product can form.

4 C(s) + 2 H 2 (g) CH 4 (g) + 18 kcal In an exothermic reaction, heat is released. the energy of the products is less than the energy of the reactants. heat is a product. Exothermic Reactions Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

5 Endothermic Reactions In an endothermic reaction Heat is absorbed. The energy of the products is greater than the energy of the reactants. Heat is a reactant (added). Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings N 2 (g) + O 2 (g) kcal 2NO(g)

6 Summary Reaction Energy Heat Type Change in Reaction Endothermic Heat absorbed Reactant Exothermic Heat released Product

7 Learning Check Identify each reaction as 1) exothermic or 2) endothermic. A. N H 2 2 NH kcal B. CaCO kcalCaO + CO 2 C. 2 SO 2 + O 2 2 SO 3 + heat

8 Solution Identify each reaction as 1) exothermic or 2) endothermic. 1 A. N H 2 2 NH kcal 2 B. CaCO kcal CaO + CO 2 1 C. 2 SO 2 + O 2 2 SO 3 + heat

9 Rate of Reaction Reaction rate is the speed at which reactant is used up. is the speed at which product forms. increases when temperature rises because reacting molecules move faster providing more colliding molecules with energy of activation.

10 Reaction Rate and Catalysts A catalyst increases the rate of a reaction. lowers the energy of activation. is not used up during the reaction.

11 Learning Check State the effect of each on the rate of reaction as: 1) increases 2) decreases3) no change A. increasing the temperature. B. removing some of the reactants. C. adding a catalyst. D. placing the reaction flask in ice. E. increasing the concentration of one of the reactants.

12 Solution State the effect of each on the rate of reaction as: 1) increases 2) decreases3) no change 1 A. increasing the temperature. 2 B. removing some of the reactants. 1 C. adding a catalyst. 2 D. placing the reaction flask in ice. 1 E. increasing the concentration of one of the reactants.

13 Learning Check Indicate the effect of each factor listed on the rate of the following reaction as 1) increases 2) decreases 3) none. 2 CO(g) + O 2 (g) 2 CO 2 (g) A. raising the temperature B. adding O 2 C. adding a catalyst D. lowering the temperature

14 Solution Indicate the effect of each factor listed on the rate of the following reaction as 1) increases 2) decreases 3) none: 2CO(g) + O 2 (g) 2CO 2 (g) 1 A. raising the temperature 1 B. adding O 2 1 C. adding a catalyst 2 D. lowering the temperature

15 Summary of Factors That Increase Reaction Rate