Skip to main content
Super TutorResources
Chapter 6 of 9
QuestionsNotesFlashcardsSummaryFormulasQuizConceptsSyllabusPlan
Revision Notes

Equilibrium

ICSE · Class 11 · Chemistry

Quick revision notes for Equilibrium — ICSE Class 11 Chemistry. Key concepts, formulas, and definitions for last-minute revision.

81 questions38 flashcards5 concepts

Interactive on Super Tutor

Studying Equilibrium? Get the full interactive chapter.

Quizzes, flashcards, AI doubt-solver and a step-by-step study plan — built for revision notes and more.

Try Super Tutor — Free

1,000+ Class 11 students started this chapter today

A comparison illustrating why physical equilibrium (like liquid-vapor equilibrium) can only be achieved in a closed system, not an open one, due to the containment of matter.
Super Tutor

This is just one of 24+ visuals inside Super Tutor's Equilibrium chapter

Explore the full set

Key Topics to Revise

1

1. Physical and Chemical Equilibrium

  • A large number of chemical reactions do not go to completion and attain a state of equilibrium after some time.
  • Equilibrium is dynamic: both forward and backward processes continue at the same rate.
  • The symbol for equilibrium is ⇌, read as reversible arrow.
2

2. Henry's Law and Dissolution of Gases

  • Henry's Law was given by William Henry in 1803.
  • The mass of a gas dissolved in a given mass of solvent is proportional to the pressure of the gas at equilibrium, provided the gas does not undergo chemical change.
  • Henry's law applies only to ideal gases, or real gases at low pressure.
3

3. Law of Mass Action, Equilibrium Constant, and Reaction Quotient

  • Law of mass action was given by Guldberg and Waage in 1864.
  • At constant temperature, the rate of a chemical reaction is directly proportional to the product of active masses of reacting species, each raised to its stoichiometric coefficient.
  • Equilibrium constant expresses the ratio of product active masses to reactant active masses at equilibrium.
4

4. Types of Chemical Equilibria

  • Homogeneous equilibrium means all reactants and products are in the same phase.
  • Heterogeneous equilibrium means reactants and products are in different phases.
  • Examples of homogeneous equilibria include H2(g) + I2(g) ⇌ 2HI(g), 2SO2(g) + O2(g) ⇌ 2SO3(g), and CH3COOH(l) + C2H5OH(l) ⇌ CH3COOC2H5(l) + H2O(l).

Get complete notes with diagrams and examples

Full Notes

Key Concepts

Equilibrium in physical processes appearsA reversible reaction reaches chemical equilibriumAt constant temperatureKc is written using equilibrium concentrationsQ has the same form as

Frequently Asked Questions

What are the important topics in Equilibrium for ICSE Class 11 Chemistry?
Key topics in Equilibrium include Equilibrium: Comprehensive Concept Overview, Equilibrium Concepts Overview, Process for optimizing industrial chemical equilibrium. These are the concepts ICSE Class 11 examiners draw on most — study them first, then practise related questions.
How to score full marks in Equilibrium — ICSE Class 11 Chemistry?
Understand the core concepts first, then work through the 81 practice questions available for this chapter. Revise formulas and definitions regularly, and use flashcards for quick recall before the exam.

Sources & Official References

Content is aligned to the official syllabus. Refer to the board website for the latest curriculum.

More resources for Equilibrium

All 9 chapters — ICSE Class 11 Chemistry Revision Notes

For serious students

Get the full Equilibrium chapter — for free.

Quizzes, flashcards, AI doubt-solver and a step-by-step study plan for ICSE Class 11 Chemistry.

Try Super Tutor Free
Try the full chapter — Free