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Unit 7: Equilibrium

Chemical equilibrium is central to understanding reaction processes in various settings. The dynamics of equilibrium highlight how reactions can shift in response to changes in concentration, pressure, or temperature. Key industrial applications demonstrate how equilibrium principles are applied to optimize chemical production processes, such as ammonia and sulfuric acid synthesis.

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Sections

  • 7

    Equilibrium

    This section introduces the concept of chemical equilibrium, emphasizing its significance in reactions and industrial applications.

    Learning Practice

  • 7.1

    Dynamic Equilibrium And The Equilibrium Constant

    This section introduces the concept of dynamic equilibrium in chemical reactions, including the equilibrium constant and how it is affected by changes in concentration, pressure, and temperature.

    Learning Practice

  • 7.1.1

    Reversible Reactions And Establishing Equilibrium

    This section discusses reversible reactions, dynamic equilibrium, and the differences between homogeneous and heterogeneous equilibria.

    Learning Practice

  • 7.1.2

    The Law Of Mass Action And The Equilibrium Constant (Kc)

    The Law of Mass Action establishes the relationship between the concentrations of reactants and products at equilibrium, leading to the formation of the equilibrium constant (Kc).

    Learning Practice

  • 7.1.3

    Kp: Equilibrium Constant In Terms Of Partial Pressures

    This section details the concept of the equilibrium constant Kp, which expresses equilibrium in gas-phase reactions in terms of partial pressures.

    Learning Practice

  • 7.1.4

    Calculating Equilibrium Concentrations (Ice Tables)

    This section details the ICE table method used for calculating equilibrium concentrations in chemical reactions.

    Learning Practice

  • 7.2

    Le Châtelier’s Principle

    Le Châtelier’s Principle describes how a system at equilibrium responds to changes in concentration, pressure, or temperature to re-establish equilibrium.

    Learning Practice

  • 7.2.1

    Statement Of Le Châtelier’s Principle

    Le Châtelier’s Principle states that a system at equilibrium will adjust to partially counteract any external change imposed on it.

    Learning Practice

  • 7.2.2

    Effect Of Concentration Changes

    This section details how changes in the concentrations of reactants or products affect the position of chemical equilibrium, as formulated by Le Châtelier's Principle.

    Learning Practice

  • 7.2.3

    Effect Of Pressure Changes (For Gas‐phase Equilibria)

    This section discusses how pressure changes affect gas-phase equilibria according to Le Châtelier's Principle, including how changes can shift the equilibrium position of reactions.

    Learning Practice

  • 7.2.4

    Effect Of Temperature Changes

    Temperature changes impact chemical equilibrium by altering the equilibrium constant and causing shifts in the equilibrium position.

    Learning Practice

  • 7.2.5

    Effect Of Catalysts

    Catalysts expedite the attainment of equilibrium in chemical reactions without altering the equilibrium position or value of the equilibrium constant.

    Learning Practice

  • 7.3

    Applications Of Equilibrium In Industry

    This section details how chemical industries apply equilibrium concepts to optimize production processes for ammonia, sulfuric acid, and other products.

    Learning Practice

  • 7.3.1

    Haber–bosch Process (Ammonia Synthesis)

    The Haber–Bosch process is a crucial industrial method for synthesizing ammonia, primarily used in fertilizers, emphasizing optimal conditions based on equilibrium and kinetics.

    Learning Practice

  • 7.3.2

    Contact Process (Sulfuric Acid Production)

    The Contact Process is a key method for producing sulfur trioxide and subsequently sulfuric acid through optimizing equilibrium conditions related to pressure, temperature, and catalysts.

    Learning Practice

  • 7.3.3

    Esterification (Production Of Esters)

    Esterification is the process of forming esters from carboxylic acids and alcohols, which is often utilized in industrial applications.

    Learning Practice

  • 7.3.4

    Other Industrial Equilibrium Processes

    The section discusses various industrial processes that utilize equilibrium principles, including the Ostwald Process for nitric acid production, solvent extraction methods, and carbon capture techniques.

    Learning Practice

References

Untitled document (17).pdf

Class Notes

Memorization

What we have learnt

  • Dynamic equilibrium occurs ...
  • The equilibrium constant ex...
  • Le Châtelier’s Principle pr...

Final Test

Revision Tests

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