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Kinetics and Thermodynamics

Kinetics and Thermodynamics. Cartoon courtesy of NearingZero.net. Enthalpy and Entropy. Reactions tend to proceed in the direction that lowers the energy of the system (H, enthalpy). Reactions tend to proceed in the direction that increases the disorder of the system (S, entropy). Entropy.

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Kinetics and Thermodynamics

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  1. Kinetics and Thermodynamics Cartoon courtesy of NearingZero.net

  2. Enthalpy and Entropy Reactions tend to proceed in the direction that lowers the energy of the system (H, enthalpy). Reactions tend to proceed in the direction that increases the disorder of the system (S, entropy). Entropy Enthalpy

  3. Endothermic Reactions

  4. Exothermic Reactions

  5. A Bomb Calorimeter

  6. A Cheaper Calorimeter

  7. Specific Heat The amount of heat required to raise the temperature of one gram of substance by one degree Celsius.

  8. Calculations involving Specific Heat OR cp = Specific Heat q = Heat lost or gained T = Temperature change m = Mass

  9. J J/gx0C J/g J/g

  10. Table of Specific Heats

  11. Molar Heat of Fusion The energy that must be absorbed in order to convert one gram of solid to liquid at its melting point. The energy that must be removed in order to convert one gram of liquid to solid at its freezing point.

  12. The heat of fusion is the heat needed to melt 1 gram of a solid at constant T. The quantity of heat that is absorbed during fusion or melting is released during solidification or freezing. • q = mHf   • m = mass • Hf = heat of fusion • Example • The heat of fusion of water is 334 J/g. Therefore, to melt 1 g of ice at  0 oC 334 J are required . • Problems   • 1. What is the heat needed to melt 100.0 grams of ice? • 2. How many grams of ice can be melted with 668 J? • 3. What is the heat of fusion of substance X if 200.0 J are required to melt 10.0 g of X? • 4. What is the heat released when 2.0 kg of water freezes? 33400.0J 2g 20.0 g/J 668,000.0 J

  13. Heat of Vaporization The energy that must be absorbed in order to convert one gram of liquid to gas at its boiling point. The energy that must be removed in order to convert one gram of gasto liquid at its point of condensation.

  14. The heat of vaporizationis the heat needed to vaporize 1 gram of a liquid at constant T. The quantity of heat that is absorbed during vaporization is released during condensation. • Heat: q = mHv   • q = heat • m = mass • Hv = heat of vaporization • Example • The heat of vaporization of water is 2260 J/g. Therefore, to vaporize 1 g of water at 100 oC 2260 J are required . • Problems  • 1. What is the heat needed to vaporize 1000.0 grams of water? • 2. How many grams of water can be vaporized with 6780 J? • 3. What is the heat of vaporization of substance Y if 500.0 J are required to vaporize 100.0 g of X? • 4. What is the heat released when 2000.0 mg of water condenses?

  15. Chemical Kinetics Key Idea: Molecules must collide to react. The area of chemistry that concerns reaction rates. However, only a small fraction of collisions produces a reaction. Why?

  16. Collision Model Collisions must have enough energy to produce the reaction (must equal or exceed the activation energy). Orientation of reactants must allow formation of new bonds.

  17. Reaction Mechanism • The series of stepsby which a chemical • reaction occurs. • A chemical equation does not tell us • howreactants become products • It is asummaryof theoverallprocess. Example: has many steps in the reaction mechanism

  18. Rate-Determining Step In a multi-step reaction, the slowest stepis the rate-determining step. It therefore determines the rate of reaction.

  19. Catalysis • Catalyst: A substance that speeds up a reaction without being consumed • Enzyme: A large molecule (usually a protein) that catalyzes biological reactions. • Homogeneous catalyst: Present in the same phase as the reacting molecules. • Heterogeneous catalyst: Present in a different phase than the reacting molecules.

  20. Factors Affecting Rate • Temperature • Increasing temperature always makes the molecules or atoms move faster thus increasing the opportunity for collisions to occur. Surface Area Increasing surface area increases the rate of a reaction • ConcentrationIncreasing the concentration of the reactants will increase the frequency of collisions between the two reactants. Increasing concentration USUALLY increases the rate of a reaction • Presence of Catalysts

  21. Catalysts Increase the Number of Effective Collisions

  22. Endothermic Reaction witha Catalyst

  23. Exothermic Reaction with a Catalyst

  24. Chemical Equilibrium Reversible Reactions: A chemical reaction in which the products can react to re-form the reactants Chemical Equilibrium: When the rate of the forward reaction equals the rate of the reverse reaction and the concentration of products and reactants remains unchanged 2HgO(s)  2Hg(l) + O2(g) Arrows going both directions (  ) indicates equilibrium in a chemical equation

  25. LeChatelier’s Principle When a system at equilibrium is placed under stress, the system will undergo a change in such a way as to relieve that stress.

  26. Le Chatelier Translated: When you take something away from a system at equilibrium, the system shifts in such a way as to replace what you’ve taken away. When you add something to a system at equilibrium, the system shifts in such a way as to use up what you’ve added.

  27. LeChatelier Example #1 A closed container of ice and water at equilibrium. The temperature is raised. Ice + Energy  Water The equilibrium of the system shifts to the _______ to use up the added energy. right

  28. LeChatelier Example #2 A closed container of N2O4 and NO2 at equilibrium. NO2 is added to the container. N2O4 (g) + Energy  2 NO2(g) The equilibrium of the system shifts to the _______ to use up the added NO2. left

  29. LeChatelier Example #3 A closed container of water and its vapor at equilibrium. Vapor is removed from the system. water + Energy  vapor The equilibrium of the system shifts to the _______ to replace the vapor. right

  30. LeChatelier Example #4 A closed container of N2O4 and NO2 at equilibrium. The pressure is increased. N2O4 (g) + Energy  2 NO2(g) The equilibrium of the system shifts to the _______ to lower the pressure, because there are fewer moles of gas on that side of the equation. left

  31. Practice EOC Problems

  32. Practice EOC Problems

  33. Practice EOC Problems

  34. Practice EOC Problems

  35. Practice EOC Problems

  36. Practice EOC Problems

  37. Practice EOC Problems

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