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Cambridge AS & A Level Chemistry

7.1Chemical equilibria: reversible reactions, dynamic equilibrium

Chemical equilibria: reversible reactions, dynamic equilibrium in Cambridge AS & A Level Chemistry: what the syllabus expects you to know, the learning objectives and how to practise.
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Learning objectives

What the syllabus expects you to be able to do.

  1. 7.1.1Explain reversible reaction and dynamic equilibrium, and why a closed system is needed.
  2. 7.1.2State Le Chatelier's principle.
  3. 7.1.3Deduce qualitatively the effect of temperature, concentration, pressure or a catalyst on an equilibrium.
  4. 7.1.4Write Kc expressions.
  5. 7.1.5Use mole fraction and partial pressure.
  6. 7.1.6Write Kp expressions (the Kp-Kc relationship is not required).
  7. 7.1.7Calculate with Kc and Kp (no quadratic equations).
  8. 7.1.8Calculate the quantities present at equilibrium from given data.
  9. 7.1.9State which changes affect the value of an equilibrium constant.
  10. 7.1.10Describe and explain the conditions of the Haber and Contact processes.

Lessons

  • Dynamic equilibrium and Le Chatelier's principle

    40 min

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  • Equilibrium constants Kc and Kp

    50 min

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  • The Haber and Contact processes

    45 min

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Sample question

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Chemical equilibria: reversible reactions, dynamic equilibrium: sample question

1 mark

The equilibrium NX2OX4(g)⇌2 NOX2(g)\ce{N2O4(g) <=> 2NO2(g)} is set up in a sealed syringe; NX2OX4\ce{N2O4} is colourless and NOX2\ce{NO2} is brown. The forward reaction is endothermic. Which change moves the position of equilibrium to the right?

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