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HSC Chemistry

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  1. Module 5: Equilibrium and Acid Reactions
    5.1 Static and Dynamic Equilibrium
    5 Topics
  2. 5.2 Factors that Affect Equilibrium
    2 Topics
  3. 5.3 Calculating the Equilibrium Constant
    2 Topics
  4. 5.4 Solution Equilibria
  5. Module 6: Acid/Base Reactions
    6.1 Properties of Acids and Bases
    7 Topics
  6. 6.2 Using Brønsted–Lowry Theory
    2 Topics
  7. 6.3 Quantitative Analysis
    1 Topic
  8. Module 7: Organic Chemistry
    7.1 Nomenclature
    2 Topics
  9. 7.2 Hydrocarbons
    2 Topics
  10. 7.3 Products of Reactions Involving Hydrocarbons
  11. 7.4 Alcohols
    1 Topic
  12. 7.5 Reactions of Organic Acids and Bases
  13. 7.6 Polymers
    2 Topics
  14. Module 8: Applying Chemical Ideas
    8.1 Analysis of Inorganic Substances
    3 Topics
  15. 8.2 Analysis of Organic Substances
  16. 8.3 Chemical Synthesis and Design
  17. Working Scientifically
    Working Scientifically Overview
    1 Topic

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Lesson 1, Topic 4
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Collision Theory and Reaction Rate

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In an endothermic process, the activation energy for the forward reaction is much greater than the activation energy for the reverse reaction. Heating the system increases the forward rate at which reactants are turned into products. The equilibrium shifts to the right as more products form.

In an exothermic process, the activation energy for the reverse reaction is much greater than for the forward reaction. If the system is heated the rate of the reverse reaction increases and more reactants form. The equilibrium shifts to the left.

The rate of reaction is dependent on the frequency of collision between reacting particles. The greater concentration of the reacting particles, the greater the collision frequency. Over time the reacting particles are consumed and their concentration decreases.

Equilibrium is achieved when the rate of the forward reaction equals the rate of the reverse reaction.