Chemical Equilibrium

Name: Chemical Equilibrium
Rating: 1.7 (2 reviews)

Reversible and irreversible reactions

Created byVinay Arya

Last updated 10/2021

English

What you'll learn

The students will have a clear vision about the Forward Reactions
The students will have a clear vision about the Backward Reactions.
The learners will become confident in Reversible reaction concept.
The learners will know about Law of Mass Action.

Course content

1 section • 17 lectures • 3h 36m total length

Contents of Equilibrium8:41
Explore the contents of chemical equilibrium, including physical and chemical processes, mass action, equilibrium constants (Kc, Kp), and the principle based on concentration, temperature, pressure, and catalyst changes.
Equilibrium in Physical Process16:33
Explore equilibrium in physical processes, where solid–liquid, liquid–gas, and solution systems reach dynamic balance as forward and backward rates equalize. Learn how saturation and vapor pressure govern evaporation and condensation.
Equilibrium in Chemical Process17:15
Explains chemical equilibrium as a dynamic balance with forward and backward reactions at equal rates in reversible processes in closed systems. Highlights homogeneous and heterogeneous equilibria.
Law of Mass Action9:11
The law of mass action states that rate equals the product of reactant concentrations raised to their powers; at constant temperature, forward and backward rates reach equilibrium, yielding equilibrium constant.
Characteristics of Equilibrium Constant K13:51
Explore how the equilibrium constant K characterizes a reaction, depending on temperature and reactant nature, while independent of initial concentrations and inert materials, and relate Kc to Kp in gases.
Relation between KP and KC11:42
Explore the relation between KP and KC, deriving how KP converts to KC in chemical equilibrium and applying to gas-phase reactions A + B ⇄ C + D.
Le Chatelier’s Principle12:41
Explore Le Chatelier’s principle and how changing concentration, pressure, or temperature shifts a chemical equilibrium toward the direction that minimizes disturbance, with ammonia synthesis as an illustrative example.
Temperature Effect11:56
Examine how temperature and pressure influence forward and backward reactions in chemical equilibrium, with examples like the Haber process illustrating shifts toward products or reactants.
Effect of Catalyst on Equilibrium10:39
Explore how catalysts accelerate both forward and reverse reactions without changing the equilibrium, while inert gases, temperature, and pressure shape the system via Le Chatelier's principle.
Ionic Equilibrium11:25
Explore ionic equilibrium, distinguishing strong and weak electrolytes, defining the degree of ionization, applying the dilution law, and analyzing the common ion effect on dissociation.
Theory of Acid and Base15:42
The lecture reviews Arrhenius, Bronsted-Lowry and Lewis theories of acids and bases, contrasts strong and weak acids, and explains proton transfer and electron-pair donation in neutralization.
Relative strength of weak acids and bases19:13
Explore the relative strength of weak acids and bases in chemical equilibrium using dissociation constants and the degree of dissociation. Learn how these concepts determine pH and conjugate acid-base relationships.
Hydrolysis of Salts12:37
Explore the hydrolysis of salts in water, classified by weak or strong acids and bases, and learn how concentration and dilution govern the extent of hydrolysis across four cases.
Strong Acid and Weak Acid9:27
Learn hydrolysis of strong acids with weak acids and salts, derive equilibrium expressions for dissociation, and calculate pH using Kw and related concentrations.
Salt of a Weak Base and a Strong Acid9:59
Analyze the hydrolysis of salts from a weak base and a strong acid to predict solution acidity via water equilibrium and ion concentrations.
Buffer Solutions11:26
Learn how buffer solutions resist pH change, with acidic buffers (weak acid and strong base) and basic buffers (weak base and strong acid), using Henderson's equation and common ion effect.
Solubility Product14:34
Explore the solubility product in chemical equilibrium, showing how ionic product relates to Ksp to indicate saturated, unsaturated, or supersaturated solutions. Learn how precipitation arises from exceeding Ksp.

Requirements

The learner should be aware of types of reactions.

Description

It is an experimental fact that most of the process including chemical reactions, when

carried out in a closed vessel, do not go to completion. They proceed to some extent

leaving considerable amounts of reactants & products. When such stage is reached in

a reaction, it is said that the reaction has attained the state of equilibrium. Equilibrium

represents the state of a process in which the properties like temperature, pressure,

concentration etc. of the system do not show any change with passage of time. In all

processes which attain equilibrium, two opposing processes are involved. Equilibrium

is attained when the rates of the two opposing processes become equal.

If the opposing processes involve only physical changes, the equilibrium is called

Physical Equilibrium. If the opposing processes are chemical reactions, the

equilibrium is called Chemical Equilibrium.

If you add more and more salt in water taken in a container of a glass and stirred

with a glass rod, after dissolving of some amount. You will find out no further

salt is going to the solution and it settles down at the bottom. The solution is now

said to be saturated and in a state of equilibrium. At this stage, many molecule of

salt from the undissolved salt go into the solution (dissolution) and same amount

of dissolved salt are deposited back (Precipitation).

Thus, at equilibrium rate of dissolution is equal to rate of precipitation.

Who this course is for:

Biggane and eleventh standard students.