Chemical Equilibrium FULL CHAPTER | Class 11th Physical Chemistry | Arjuna NEET

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Equilibrium in reversible reactions depends on equal forward and backward rates, with equilibrium constants crucial for maintaining stability. Changes in pressure can disturb equilibrium, shifting the reaction towards the side with fewer gas moles.

Insights

Reversible reactions involve both forward and backward reactions, reaching equilibrium when their rates are equal.
Equilibrium constants are crucial, calculated based on the ratio of product to reactant concentrations.
Concentration plays a vital role in reversible reactions, affecting forward and backward rates.
Le Chatelier's principle dictates that reducing a reactant prompts a forward reaction, while increasing it triggers a backward reaction.
Equilibrium shifts towards the side with fewer moles of gas when pressure is increased, influencing reaction direction.

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Recent questions

What are reversible reactions?
Reversible reactions involve both forward and backward reactions occurring.
How is equilibrium constant calculated?
The equilibrium constant is determined by the ratio of product concentration to reactant concentration.
What is the role of concentration in reversible reactions?
Concentration is crucial in reversible reactions, affecting forward and backward rates.
How do catalysts impact equilibrium?
Catalysts can significantly affect reaction rates without disturbing equilibrium.
What happens when pressure changes in a reaction?
Changes in pressure can disturb equilibrium, shifting towards the side with more gas moles.

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Summary

00:00

"Understanding Reversible and Irreversible Chemical Reactions"

There are two types of reactions: reversible and irreversible.
Reversible reactions involve both forward and backward reactions taking place.
Equilibrium is reached when the forward and backward reactions are equal.
Reversible reactions occur when reactants and products are distributed equally.
Equilibrium constant is calculated by the ratio of product concentration to reactant concentration.
The equilibrium constant increases with higher product concentration and decreases with higher reactant concentration.
Irreversible reactions result in a high equilibrium constant due to excessive product formation.
Attainment of equilibrium in reversible reactions is when forward and backward rates are equal.
The rate of a reaction is proportional to the active mass of reactive substances.
The rate of a chemical reaction is directly proportional to the active mass and stoichiometric coefficients of the reactants.

14:36

Understanding Equilibrium Reactions and Rate Constants

Beta Molar is used instead of active mass in a story to simplify understanding.
Concentration is crucial in reversible reactions, determining forward and backward rates.
The rate of reaction is directly proportional to the concentration of reacting species.
Stoichiometric coefficient plays a vital role in determining reaction rates.
The formula for Dr. Mass Action includes active mass and molar concentration.
Rate constants remain constant regardless of concentration changes.
Rate constants depend on temperature and the nature of the reaction.
Equilibrium is reached when forward and backward rates are equal.
Equilibrium constant is calculated based on product and reactant concentrations.
Solids and liquids are considered constants in equilibrium calculations.

30:37

"Equilibrium Constant: Key to Chemical Stability"

Equilibrium constant is crucial in chemical reactions
Equilibrium constant is calculated by multiplying the equilibrium constants of individual reactions
Equilibrium constant is determined by the concentration of products divided by the concentration of reactants
Equilibrium constant of a reaction can be altered by changing reactant or product concentrations
Equilibrium constant remains constant if temperature and nature of the reaction are unchanged
Disturbing equilibrium prompts the reaction to readjust to reach equilibrium again
Equilibrium constant of 1 signifies a stable reaction at equilibrium
Changing reactant or product concentrations leads the reaction back to equilibrium
Equilibrium constant is a key factor in maintaining stability in chemical reactions
Understanding the concept of equilibrium constant aids in predicting and managing chemical reactions

46:35

Equilibrium Constants Determine Reaction Direction

Value is determined by equilibrium in a reaction
Removing a component disrupts equilibrium
Equilibrium constant remains constant
Calculations involve concentrations at equilibrium
Determining the direction of a reaction based on equilibrium
New equilibrium constant is calculated
Calculating concentrations at new equilibrium
Understanding the significance of equilibrium constant
Shift in equilibrium towards products
Maintaining equilibrium by adjusting reactants and products

01:02:00

Reactant Amount Influences Equilibrium Shifts

To achieve a forward reaction, increase the reactant amount.
Equilibrium is disturbed when the amount of reactant is reduced.
External changes lead to the system adjusting itself to maintain equilibrium.
The Le Chatelier's principle dictates that reducing a reactant prompts a forward reaction.
Increasing the reactant amount triggers a backward reaction.
Calculations are crucial to determine the direction of the reaction when multiple changes occur.
The reaction quotient helps in understanding the equilibrium shift due to changes.
Calculations are essential to determine the new equilibrium composition after adding reactants.
The equilibrium composition is altered by adding reactants, leading to a shift in the reaction direction.
The value of x in equilibrium calculations indicates the extent of reactant or product presence.

01:16:34

Equilibrium Constant: Gas Pressure and Moles

Tu four four minus one is 3/2
The value of 3/2 is equal to the forest
The square of 3/2 will be equal to one
The value of A will be 4.5 moles
The equilibrium is disturbed by adding two more items
The equilibrium constant is expressed in terms of partial pressure of gases
The unit of the equilibrium constant is the atmosphere's power delta MG
Delta MG is the sum of moles of gases on the product side minus the reactant side
The relation between A gas and C gas in terms of partial pressures
The power of concentration is one in the equilibrium constant formula

01:32:29

Chemistry: Equilibrium, Concentration, and Dating

NIT being held allows for dating
The formula for the concentration is the number of moles divided by volume
Concentration is calculated by converting the number of moles and volume into liters
The relationship between partial pressure and concentration is discussed
The equation for partial pressure and concentration is explained
Delta ng is defined as the difference in the number of moles of gases in the product and reactant
The relationship between equilibrium constants and reactions is detailed
The formula for equilibrium constant is provided
The concept of degree of advancement of a reaction is introduced
The calculation of degree of dissociation (alpha) is explained using initial and reacted moles

01:49:13

Gas Equilibrium Shift: Writing, Calculation, Pressure, Moles

Writing is emphasized, with the mention of IBM Pay One for completion.
Calculation of mass fraction is explained as 1 - Alpha / Total.
The formula for malls calculation is detailed as 2 alpha / 1 + 2 alpha.
Instructions on calculating partial pressures for different gases are provided.
The expression for cup in terms of total pressure and degree of dissociation is elaborated.
The impact of temperature on total pressure is discussed.
A mathematical equation for expressing alpha in terms of cup and total pressure is presented.
The effect of pressure on equilibrium is explained, with a focus on total pressure calculation.
The concept of pressure affecting equilibrium shift towards the side with fewer moles of gas is highlighted.
The importance of understanding gas moles and pressure in determining equilibrium shift is emphasized.

02:06:33

Pressure Changes Shift Equilibrium Towards Fewer Moles

Equilibrium shifts towards the side with fewer moles of gas when pressure is increased.
Decreasing pressure disturbs equilibrium, causing a shift towards the side with lower gas moles.
Delta G zero signifies equilibrium, with no shift if moles are equal on both sides.
Positive delta N indicates a shift towards the side with more gas moles when pressure is increased.
Calculating equilibrium constant involves considering partial pressures of gases at equilibrium.
Adding ammonia until its pressure doubles affects the equilibrium, leading to a shift in pressures of all gases involved.
The total pressure at the new equilibrium is determined by the sum of partial pressures of all gases.
The equilibrium constant remains constant despite changes in pressures due to added reactants.
Calculating the new equilibrium partial pressures involves using the equilibrium constant and known values.
The final equilibrium total pressure is found by summing the partial pressures of all gases at the new equilibrium.

02:22:41

Gas Equilibrium Calculations and Molar Mass

The sum of the partial pressure of NH3 and CO2 is 16, and if it is 1, then it is 17.
Equilibrium is reached when the atmosphere is considered, affecting the partial pressure.
Questions should be approached by considering changes in equilibrium conditions.
Calculations involve determining the pressure of NH3 when CO2 is added.
The total pressure of gases in a container at equilibrium is calculated based on their partial pressures.
The average molar mass of a gas mixture can be found by multiplying the molar mass of each gas by its moles and dividing by the total moles.
Two methods are presented for calculating the average molar mass, one involving individual gas masses and moles, and the other based on conservation of mass.
The conservation of mass principle is applied to equate initial and final masses in a reaction.
The average molar mass calculation is demonstrated through a reaction involving O3 and O2 gases.
The degree of dissociation (alpha) in a reaction can be determined by solving equations based on molar masses and moles.

02:37:29

Temperature Effects on Equilibrium Reactions and Color

Molar mass of O2: Mole of O3+ equals mole of O2, formula can be used.
Equilibrium: Formula applicable only at equilibrium, shift in reaction direction.
Exothermic Reaction: Delta Ha negative, reaction shifts to product side.
Endothermic Reaction: Delta Ha positive, reaction shifts to reactant side.
Equilibrium Constant: Increases with temperature for endothermic, decreases for exothermic.
Clausius Equation: Relates equilibrium constants at different temperatures.
Rate Constant: Increases with temperature, affecting equilibrium.
Calculation: Ln of Kp2/Kp1 = Delta Ha/R * (1/T1 - 1/T2) for temperature change.
Experiment Questions: Exothermic reactions shift to product side, affecting color changes.
Temperature Effects: Increasing temperature intensifies color, decreasing reduces intensity.

02:53:15

Impact of Temperature and Catalysts on Equilibrium

Temperature increase leads to more dissociation and a shift in equilibrium towards the left side, intensifying the brown color.
Catalysts at equilibrium can significantly impact reaction rates, with positive catalysts speeding up reactions and maintaining equilibrium.
Catalysts can affect both forward and backward reactions proportionally, disturbing equilibrium if not balanced.
The addition of a catalyst does not affect equilibrium but accelerates the reaction rate.
Standard Gibbs Free Energy and Equilibrium Constant are related, with Delta G Note equaling -RTlnK at equilibrium.
The spontaneity of a reaction is determined by Delta G, with negative values indicating spontaneity.
The addition of an inert gas at constant volume does not affect equilibrium as the gases do not react.
Adding an inert gas at constant pressure also does not alter equilibrium as the partial pressures remain constant.
The total pressure in a container remains constant when adding an inert gas at constant pressure.
The equilibrium is undisturbed when adding an inert gas at constant pressure, as long as the total pressure is maintained.

03:09:30

Maintaining Pressure in Gas Equilibrium Reactions

Constant pressure conditions must be maintained at 3 atmospheres.
The total pressure is now P Plus Plus, with P b plus P o equalling tu.
Under constant pressure conditions, if the pressure is 180, the pressure of both gases together must be 3 atmospheres.
Equilibrium is maintained even if gas is added, as long as the pressure remains constant.
If pressure changes, the equilibrium is disturbed, shifting towards the side with more moles of gas.
Adding inert gas at constant pressure decreases the pressure, causing the equilibrium to shift towards the side with more moles of gas.
The equilibrium will move towards the side with more moles of gas if pressure decreases.
If the pressure decreases, the equilibrium will shift towards the side with more moles of gas.
The addition of inert gas at constant pressure does not affect the equilibrium.
Adding gases at constant volume does not affect the equilibrium, as the pressure decreases towards the side with more moles of gas.

03:24:36

Determining Equilibrium Constants for Reaction Prediction

Equilibrium constant is determined by halving the power of the original reaction constant.
The value of equilibrium constant is crucial in predicting the direction of a reaction.
A high equilibrium constant indicates a reaction favoring product formation.
The equilibrium constant value of 10^12 signifies a reaction with a high forward tendency.
Exothermic reactions require lower temperatures for forward reactions.
Pressure influences reactions with fewer gas moles favoring forward movement.
The reaction quotient is essential in determining the direction of a reaction.
Equilibrium constants can be expressed in terms of partial pressures.
The hydrolysis of sucrose reaction involves calculating the equilibrium constant at a specific temperature.
Understanding reversible processes at equilibrium involves considering the change in Gibbs free energy.

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