5.4 Rates of Change Pages 169 - 174
Goal 1 Describe the 5 factors that affect reaction rates
<ul><li>Collision Theory (memorize this) </li></ul><ul><li>“ chemical reactions can only occur if  </li></ul><ul><li>parti...
<ul><li>1. Temperature </li></ul><ul><ul><li>High temp = faster reaction rate </li></ul></ul><ul><ul><li>Low temp = slower...
<ul><li>2. Surface Area </li></ul><ul><ul><li>More exposed surface area = faster </li></ul></ul><ul><ul><li>Less exposed s...
<ul><li>3. Concentrations </li></ul><ul><ul><li>Higher concentration = faster  </li></ul></ul><ul><ul><li>Lower concentrat...
<ul><li>4. Pressure </li></ul><ul><ul><li>High pressure = faster  </li></ul></ul><ul><ul><li>Low pressure = slower </li></...
<ul><li>5. Mass </li></ul><ul><ul><li>Less mass = faster </li></ul></ul><ul><ul><li>More mass = slower </li></ul></ul><ul>...
<ul><li>Summary of  5 factors </li></ul><ul><ul><li>1. Temperature </li></ul></ul><ul><ul><li>2. Surface Area </li></ul></...
Goal 2 Explain the affect a catalyst has on the rate of a reaction
<ul><li>Catalysts change the rate of a reaction </li></ul><ul><ul><li>Catalysts themselves do not change or get used up </...
<ul><li>Enzyme = biological catalyst </li></ul><ul><ul><li>Substrate = substance / reactants that are affected by enzyme <...
<ul><li>Enzymes shape specific like a “lock & key” </li></ul><ul><ul><li>The enzyme “catalase”  only breaks down hydrogen ...
Goal 3 Explain chemical equilibrium
<ul><li>Reversible reactions </li></ul><ul><ul><li>SOME reactions are reversible </li></ul></ul><ul><ul><li>reversible rea...
<ul><li>Reversible reactions in Equilibrium system </li></ul><ul><ul><li>will be in equilibrium </li></ul></ul><ul><ul><li...
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5.4 Lecture

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5.4 Lecture

  1. 1. 5.4 Rates of Change Pages 169 - 174
  2. 2. Goal 1 Describe the 5 factors that affect reaction rates
  3. 3. <ul><li>Collision Theory (memorize this) </li></ul><ul><li>“ chemical reactions can only occur if </li></ul><ul><li>particles collide with enough energy to </li></ul><ul><li>result in activation” </li></ul>
  4. 4. <ul><li>1. Temperature </li></ul><ul><ul><li>High temp = faster reaction rate </li></ul></ul><ul><ul><li>Low temp = slower reaction rate </li></ul></ul><ul><ul><li>Why?.... collisions </li></ul></ul>
  5. 5. <ul><li>2. Surface Area </li></ul><ul><ul><li>More exposed surface area = faster </li></ul></ul><ul><ul><li>Less exposed surface area = slower </li></ul></ul><ul><ul><li>Why?.... collisions </li></ul></ul><ul><ul><li>Diet coke and Mentos ?? </li></ul></ul>
  6. 6. <ul><li>3. Concentrations </li></ul><ul><ul><li>Higher concentration = faster </li></ul></ul><ul><ul><li>Lower concentration = slower </li></ul></ul><ul><ul><li>Why?.... collisions </li></ul></ul>
  7. 7. <ul><li>4. Pressure </li></ul><ul><ul><li>High pressure = faster </li></ul></ul><ul><ul><li>Low pressure = slower </li></ul></ul><ul><ul><li>Why?.... collisions </li></ul></ul>
  8. 8. <ul><li>5. Mass </li></ul><ul><ul><li>Less mass = faster </li></ul></ul><ul><ul><li>More mass = slower </li></ul></ul><ul><ul><li>Why?.... collisions </li></ul></ul>
  9. 9. <ul><li>Summary of 5 factors </li></ul><ul><ul><li>1. Temperature </li></ul></ul><ul><ul><li>2. Surface Area </li></ul></ul><ul><ul><li>3. Concentration </li></ul></ul><ul><ul><li>4. Pressure </li></ul></ul><ul><ul><li>5. Mass </li></ul></ul>
  10. 10. Goal 2 Explain the affect a catalyst has on the rate of a reaction
  11. 11. <ul><li>Catalysts change the rate of a reaction </li></ul><ul><ul><li>Catalysts themselves do not change or get used up </li></ul></ul><ul><ul><li>Slows a reaction = Inhibitor </li></ul></ul>
  12. 12. <ul><li>Enzyme = biological catalyst </li></ul><ul><ul><li>Substrate = substance / reactants that are affected by enzyme </li></ul></ul>
  13. 13. <ul><li>Enzymes shape specific like a “lock & key” </li></ul><ul><ul><li>The enzyme “catalase” only breaks down hydrogen peroxide </li></ul></ul>Hydrogen peroxide  water + oxygen
  14. 14. Goal 3 Explain chemical equilibrium
  15. 15. <ul><li>Reversible reactions </li></ul><ul><ul><li>SOME reactions are reversible </li></ul></ul><ul><ul><li>reversible reactions shown by </li></ul></ul>CaCO 3 CaO + CO 2
  16. 16. <ul><li>Reversible reactions in Equilibrium system </li></ul><ul><ul><li>will be in equilibrium </li></ul></ul><ul><ul><li>Equal amounts going both ways </li></ul></ul>CaCO 3 CaO + CO 2
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