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Chemical Kinetics & Collision Theory

Chemical Kinetics & Collision Theory. Honors Chemistry Unit 16 Daily 1 Lecture. Then and Now…. Previous Unit: Will a reaction occur? Current Unit: How fast does a reaction occur?. Key Questions. How do you measure the speed, or rate, of a reaction? vs.

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Chemical Kinetics & Collision Theory

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  1. Chemical Kinetics & Collision Theory Honors Chemistry Unit 16 Daily 1 Lecture

  2. Then and Now… Previous Unit: Will a reaction occur? Current Unit: How fast does a reaction occur?

  3. Key Questions • How do you measure the speed, or rate, of a reaction? vs. 2. What factors influence how fast a reaction occurs?

  4. Key Question #1What is Rate? • How fast something takes place • Speed = distance/time If a car travels 30 miles in ½ hour, what is it’s speed?

  5. A Tale of Two Cars

  6. Reaction Rates • A measure of how fast a reaction occurs, or how something changes during a given time period. • How can you measure the speed of the following reaction: C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g) …measure how quickly the mass of solid glucose decreases …measure how quickly the gases (CO2(g) & H2O(g)) form

  7. Reaction Rates (cont.) Mg(s) + 2HCl(aq)  H2(g) + MgCl2(aq)

  8. Reaction Rates (cont.) • Other possible things that could be measured, depending on the reaction: • change in pressure as gases are formed or used up • change in volume as gases are formed or used up • change in mass as solid is formed or used up • change in temperature • change in conductivity • change in pH • change in color ex) AgNO3(aq) + Cu(s)  CuNO3(aq) + Ag(s)

  9. In a Nutshell… reaction rate = amount of product formed time interval Or… reaction rate = amount of reactant used time interval Or… reaction rate = change in concentration time interval product time reactant time

  10. Key Question #2What Affects Rates? Collision Theory: • Particles must collide for reactions to occur • Rate depends on the frequency of collisions TO SUCCEED, collisions must have: • Sufficient energy • Proper orientation

  11. Increasing Chances for Successful Collisions • Temperature • Concentration • Surface Area • Catalysts • Nature of Reactants

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