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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 3, Topic 1
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The Equilibrium Constant Expression

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The position or extent of a chemical equilibrium can be expressed quantitatively using the equilibrium constant (Keq).

The equilibrium constant may be written as the following, which is based on the ratio of products to reactants of an equilibrium system at a specific temperature:

K_{\text {eq}} = \frac{ [\text{products}]}{[\text{reactants}] }

But more specifically, it is calculated using the equilibrium constant expression. For the reaction below:

a\text A + b\text B ⇌ c\text C + d\text D

the equilibrium expression is:

K_{\text{eq}} = \frac{[\text C]^c[\text D]^d}{[\text A]^a[\text B]^b}

A change in temperature is the only factor that will cause the equilibrium constant to change. Factors such as pressure, concentration and volume will simply affect the position of equilibrium.