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- Chemical Equilibrium. In a chemical reaction chemical equilibrium is defined as the state at which there is no further change in concentration of reactants and products.
- Equilibrium in Physical Processes. (i) Solid-Liquid Equilibrium: The equilibrium is represented as. Rate of melting of ice = Rate of freezing of water. The system here is in dynamic equilibriums and following can be inferred.
- Equilibrium involving Dissolution of Solid in Liquid. Solution: When a limited amount of salt or sugar or any solute dissolves in a given amount of water solution is formed.
- Equilibrium between a Gas and its Solution in Liquid. This type of equilibrium can be seen by the following example: Let us consider a sealed soda water bottle in which C02 gas is dissolved under high pressure.
Download free study material and video tutorials for Chemical Equilibrium Class 11 from eSaral, a platform for IIT JEE and NEET preparation. Learn the concepts, key points and examples of Chemical Equilibrium with top expert IITian Faculties.
Learn about chemical equilibrium, the state of a system where the concentrations of reactants and products do not change with time. Explore the types, factors, examples and problems of chemical equilibrium with Byju's JEE study material.
4 days ago · Download free PDF of revision notes for CBSE Class 11 Chemistry Chapter 7 (Equilibrium) by Vedantu. Learn the basic concepts, definitions, examples, and applications of chemical equilibrium with practice questions and solutions.
- Equilibrium
- Equilibrium in Chemical Process
- Characteristics of Equilibrium State
- Law of Mass Action & Equilibrium Constant
- Equilibrium Quotient Or Mass Action Ratio
- The Le–Chatelier’S Principle
- Acids and Bases
- Hydrolysis of Salts
- Solubility and Solubility Product
- Ionic Product
- GeneratedCaptionsTabForHeroSec
Equilibrium is the state of a process in which the properties like temperature, pressure, and 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.Reversible reaction: A reaction in which not only the reactants react to form the products under certain conditions but also the products react to form reactants under the same conditions Example...Irreversible reaction: Areaction cannot take place in the reverse direction, i.e. the products formed do not react to give back the reactants under the same condition. Example: AgNO3(aq) + NaCl(aq)...Generally, a chemical equilibrium is represented as Where A, B are reactants and C, D are products.It can be attained only if the reversible reaction is carried out in closed vessel.It can be attained from either side of the reaction.A catalyst can hasten the approach of equilibrium but does not alter the state of equilibrium.It is dynamic in nature i.e. reaction does not stop but both forward and backward reactions take place at equal rate.“The rate at which a substance reacts is directly proportional to its active mass and rate of a chemical reaction is directly proportional to product of active masses of reactants each raised to a power equal to corresponding stoichiometric coefficient appearing in the balanced chemical equation”. Fore reaction Rate of reaction ∝ [A]a.[B]b or rate ...
Consider the equilibrium aA +bB cC +dD At equilibrium When the reaction is not at equilibrium this ratio is called ‘QC’ i.e., QC is the general term used for the above given ratio at any instant of time. And at equilibrium QC becomes KC. 1. If the reaction is at equilibrium, Q = Kc 2. A net reaction proceeds from left to right (forward direction) i...
Statement:
“When a chemical reaction at equilibrium is subjected to any stress, then the equilibrium shifts in that direction in which the effect of the stress is reduced.”
Effect of Addition of Inert Gases:
1. Addition of inert gas at constant volume: No effect on equilibrium. 2. Addition of inert gas at constant pressure: Equilibrium shifts in a direction where there is increase in number of moles of gases.
Effect of Change in Temperature:
1. In a system at equilibrium, both exothermic and endothermic reactions take place simultaneously. 2. Increase in temperature would shift the equilibrium in the direction of endothermic reaction. 3. Decrease in temperature would shift the equilibrium in the direction of exothermic reaction.
1. Arrhenius Definition: a. Acids give H+ions aqueous solutions. b. Bases give OH- ions in aqueous solution. 2. Bronsted – Lowry Definition: a. Acid is a proton donor . b. Base is a proton acceptor. 3. Strong and Weak Acids: a. Strong acid dissociate completely in aqueous solution. Example: HCl b. Weak acid dissociates partially in aqueous solution...
1. Salt of a Weak Acid and Strong Base: [H+] = (Kw Ka / C )1/2 2. Salt of a Weak Base and Strong Acid [H+] = (Kw / Kb C )1/2 3. Salt of a Weak Acid and Weak Base [H+] = (Kw Ka / Kb )1/2 1. Buffer Solutions:Resists change in its pH when such a change is caused by the addition of a small amount of acid or base. 1. Weak acid–Salt buffer: Formed by com...
1. Amount (moles) of the salt that has made the solution saturated per liter of solution is called the solubility of the salt. 2. For salt AB. AB ↔A+ +B- Ksp = [A+][B-] 3. Solution cannot have the product of the concentration of the ions more than KSP of the salt in solution.
a) Product of ionic concentration due to ions already present in water or from a salt. b) I.P. may be and may not be equal to Ksp. c) If ionic Product (IP) > Ksp ; precipitation takes place till I.P. equals Ksp d) If Ionic Product < Ksp; a precipitate will not be formed and the solution will be unsaturated. e) If Ionic Product = Ksp; a precipitate ...
Learn the basics of chemical equilibrium, such as physical and chemical equilibrium, reversible and irreversible reactions, homogeneous and heterogeneous equilibrium, law of mass action, equilibrium constant, and Le-Chatelier's principle. Also, explore the thermodynamics of chemical equilibrium and its applications.
Nov 13, 2022 · Chemical equilibrium. When a chemical reaction takes place in a container which prevents the entry or escape of any of the substances involved in the reaction, the quantities of these components change as some are consumed and others are formed.
Learn about chemical equilibrium, equilibrium constants, reaction quotients, Le Chatelier's principle, and Gibb's free energy. Practice with quizzes, worked examples, and unit tests.
