CHAPTER 3 ACTIVITY 5

1. CHAPTER 3 ACTIVITY 5 REACTION RATES & FACTORS AFFECTING EQUILIBRIUM

2. Activated Complex A.E. E of reactants 2H2 + O2 E E of products 2H2O Energy Diagrams Energy Reaction Progress A.E. (activation energy):minimum energy needed for a reaction to occur Activated Complex: transitional structure formed from an effective collision.

3. Not Every Collision Produces Products Reactants must: 1. Collide with the correct orientation 2. Have enough energy to produce products.

4. The Reaction Process Collision Theory: Explanation of reactions as a result of collisions. • Particles must collide • Particles must collide in the correct orientation • Collision must be energetic enough to disrupt bonds

5. Energy barrier w/o catalyst Energy barrier w catalyst Catalyst A substance that increases the rate of reaction without being used up itself in the reaction. Reactants Energy Products Reaction Progress

7. Exothermic vs. Endothermic Exothermic: • A process that loses heat to its surroundings. Fe2O3(s) + CO(g) Fe(s) + CO2(g) + 26.3 kJ Endothermic: • A process that absorbs heat from its surroundings. 2NaHCO3(s) + 129 kJ Na2CO3(s) + H2O(g) + CO2(g)

8. http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/activa2.swfhttp://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/activa2.swf

9. Is the following an example of an exothermic or endothermic reaction? Reactants Potential Energy EXOTHERMIC=energy is released Products Reaction Progress

10. Is the following an example of an exothermic or endothermic reaction? Products Potential Energy Reactants ENDOTHERMIC=energy is absorbed Reaction Progress

11. Factors Affecting Reaction Rates 1. Temperature 2. Concentration 3. Particle Size 4. Catalysts

12. Factors Affecting Reaction Rates 1. Temperature WHY Temp Rate Kinetic Energy

13. Factors Affecting Reaction Rates 2. Concentration WHY Conc. Rate More Particles increases collision frequency

14. Factors Affecting Reaction Rates 3. Particle Size WHY Particle Rate Smaller Particle Size size increases the surface area

15. Factors Affecting Reaction Rates 4. Catalyst WHY Adding a Rate Activation Energy Catalyst

16. FACTORS AFFECTING EQ.Le Chatelier’s Principle Reactions will stabilize and establish equilibrium. If this system is disturbed from equilibrium, it will shift in order to reduce the disturbance. When any of the following three things are changed, the system will change to re-establish equilibrium. • Concentration • Temperature • Pressure System @ Equilibrium R P Systems not @ Equilibrium

17. Know the Difference

18. Concentration If we add CO2, more H2CO3 will be made H2CO3CO2 + H2O If we remove CO2, more CO2 & H2Owill be made

19. Concentration If we remove H2CO3, more H2CO3will be made H2CO3CO2 + H2O If we add H2CO3, more CO2 & H2O will be made

20. Temperature 2SO2 + O2 2SO3 + heat If we add heat, more reactants will be made in order to absorb the excess heat If we remove heat, more products will be made in order to replace the heat that has been removed.

21. Pressure If we increase pressure, more products will be made (less moles) Only Gases Are Affected! N2 + 3H2 2NH3 4 moles If we decrease pressure, more reactants will be made (more moles) 2 moles

22. R = P Review Reactions will stabilize and establish equilibrium. When any of the following three things are changed, the reaction will change to re-establish equilibrium. • Concentration • Temperature • Pressure