CHEMICAL EQUILIBRIUM in 1 Shot: All Concepts, Tricks & PYQs | NEET Crash Course | Ummeed

Competition Wallah・2 minutes read

Equilibrium in chemical and ionic forms involves reversible reactions and understanding reaction rates to achieve balance. Factors like temperature, concentration changes, and catalysts influence equilibrium, with pressure shifts impacting gaseous moles and the final outcome of reactions.

Insights

  • Equilibrium involves balancing forward and backward reactions, with rates being equal.
  • Catalysts impact equilibrium by either speeding up or delaying reactions.
  • Temperature influences equilibrium, affecting the direction of reactions.
  • Pressure changes affect equilibrium position, with higher pressure favoring the side with fewer gaseous moles.

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Recent questions

  • What is chemical equilibrium?

    Chemical equilibrium occurs when the rates of forward and backward reactions are equal, leading to a constant state. It is dynamic in nature, with reactions proceeding in both directions at the same rate. At equilibrium, observables like pressure, volume, temperature, and concentration remain constant.

  • How do catalysts affect equilibrium?

    Catalysts can affect equilibrium by speeding up reactions, with positive catalysts accelerating equilibrium and negative catalysts delaying it. Negative catalysts increase activation energy, while positive catalysts decrease it, impacting the time it takes for equilibrium to be reached.

  • What is the impact of temperature on equilibrium?

    Temperature influences equilibrium; lower temperatures favor the backward reaction, while higher temperatures favor the forward reaction. Understanding how temperature affects equilibrium is crucial for predicting the direction in which a reaction will proceed.

  • How does pressure affect equilibrium?

    Pressure affects the equilibrium position in a reaction; increasing pressure shifts the equilibrium towards the side with fewer gaseous moles. To maximize product yield, keeping pressure low is recommended to push the equilibrium towards the forward direction.

  • What is the significance of volume changes in equilibrium?

    Equilibrium remains unaffected by changes in volume or the addition of inert gases at constant volume or pressure. Understanding how volume changes impact equilibrium is essential for predicting the behavior of a system under different conditions.

Related videos

Summary

00:00

"Equilibrium: Chemical and Physical Reactions Explained"

  • The lecture will cover Equilibrium in two parts, focusing on chemical and ionic equilibrium.
  • Chemical equilibrium is a short but important chapter, with potential questions in exams.
  • Reversible reactions involve products turning back into reactants, while irreversible reactions do not.
  • Examples of reversible reactions include melting ice to water and folding a paper clip.
  • Physical changes, like changing the shape of clay, are reversible, while chemical changes, like burning paper, are irreversible.
  • Equilibrium is when the rates of forward and backward reactions are equal.
  • Physical equilibrium involves no chemical changes, only changes in physical state.
  • An example of physical equilibrium is ice and water at their freezing point.
  • Liquid-gas equilibrium involves water at a specific temperature, close to its boiling or melting point.
  • Understanding equilibrium is crucial for grasping the balance between reactants and products in reactions.

20:08

"Equilibrium in Chemistry: A Dynamic Balance"

  • Water vapor is also water, just in a gaseous state, and equilibrium is reached when the rate of evaporation equals the rate of condensation.
  • Naphthalene balls are an example of solid-gas equilibrium, where some solids sublime directly into gas, like dry ice converting to carbon dioxide gas.
  • Chemical equilibrium occurs when the rates of forward and backward reactions are equal, leading to a constant state.
  • Equilibrium is dynamic in nature, with reactions proceeding in both directions at the same rate.
  • Observables like pressure, volume, temperature, and concentration remain constant at equilibrium.
  • Catalysts can affect equilibrium by speeding up reactions, with positive catalysts accelerating equilibrium and negative catalysts delaying it.
  • Negative catalysts increase activation energy, while positive catalysts decrease it, impacting the time it takes for equilibrium to be reached.
  • Equilibrium is characterized by a change in free energy, with delta G becoming zero when equilibrium is achieved.

35:46

"Equilibrium and Temperature in Gas Reactions"

  • Delta gives free energy at standard conditions, not zero.
  • N2O is a gas with a color of reddish brown.
  • Equilibrium between N2O and NO2 can be achieved at room temperature.
  • Temperature affects the equilibrium between N2O and NO2.
  • Ice can lower the temperature to convert N2O to NO2.
  • Equilibrium between N2O and NO2 can be achieved from any side.
  • Delta H is related to the temperature change in the reaction.
  • Equilibrium constant can be calculated in terms of concentration or partial pressure.
  • The universal gas constant value depends on the units used.
  • Delta ng is the change in the number of moles of gases in a reaction.

54:08

"Equilibrium values and calculations in chemistry"

  • The value of keeping one or two items is discussed, with the value increasing when more items are kept.
  • Multiplying a value by a certain factor results in a larger value.
  • Negative values occur when gaseous moles of the product are fewer than the reactants.
  • A value of zero for Delta AG indicates an equilibrium when gaseous moles of both reactants are equal.
  • Raising a value to the power of zero results in a value of one.
  • The relationship between Cape and Casey is explored, with their values becoming equal when certain conditions are met.
  • Calculations involving concentrations of PCL5, PCL3, and CL2 are detailed, leading to specific numerical results.
  • The unit of concentration is determined to be liters per mole through a series of calculations.
  • The concept of equilibrium in a chemical reaction is discussed, with the rates of forward and backward reactions being compared.
  • The restoration of equilibrium after disturbance is explained, with the rate of backward reaction increasing to restore equilibrium.

01:09:44

"Chemical Equilibrium: Concentration, Constants, and Reactions"

  • The aim is to teach and help in selection, focusing on product side and increasing concentration.
  • Concentration affects the equilibrium constant, with a specific saying about being in an angry mood.
  • The chapter on chemical equilibrium is discussed, emphasizing that easy chapters may contain challenging topics.
  • Questions often focus on good topics like aldehydes and ketones, requiring brain usage.
  • The characteristic of equilibrium constants is highlighted, with a focus on the extent of reaction.
  • The equilibrium constant depends on the concentration of reactants and products, indicating the reaction's completeness.
  • The concept of equilibrium is explained through a relatable scenario of students feeling sleepy in class.
  • The importance of active mass in equilibrium constants is discussed, emphasizing the role of pure solids and liquids.
  • The impact of temperature changes on equilibrium constants, especially in endothermic reactions, is detailed.
  • Changes in stoichiometry of reactions directly affect the equilibrium constant, with doubling or halving stoichiometric coefficients leading to specific changes in the constant's value.

01:28:30

"Equilibrium Constants: Factors and Reversal Effects"

  • Equations are added, reactants on one side and products on the other.
  • Equilibrium constant is formed by multiplying three constants.
  • Concentration of products and reactants is crucial for equilibrium.
  • Reversing equations changes equilibrium constants.
  • Doubling somatic comfort power affects equilibrium constant.
  • Reactants convert to products with high equilibrium constant.
  • Pressure and volume changes do not affect equilibrium constant.
  • Dissociation of acetic acid results in acetate and hydrogen ions.
  • Reversing equations helps find equilibrium constants.
  • Reactants increase in backward reactions, affecting equilibrium.

01:48:17

Equilibrium Constants and Concentrations in Chemistry

  • Moles are written by volume only, with a volume of 1 liter.
  • Equilibrium is reached when the value is 10^-3.
  • Questions in class focus on equilibrium constants, with examples like P4 giving P2.
  • Concentration calculations involve stoichiometric coefficients and volume.
  • Equilibrium concentration is determined by moles divided by volume.
  • Concentration of products is influenced by stoichiometric coefficients of reactants.
  • Equilibrium constants are calculated based on concentration and volume.
  • Partial pressures are considered in equilibrium calculations.
  • Numerical questions involve moles of NH3 dissociating into N2 and H2.
  • Equilibrium moles are determined by dissociation and remaining quantities.

02:08:54

Equilibrium Constants and Concentrations in Competition

  • The answer to option D is 27 times 16, related to a competition.
  • If the initial concentration of A and B is equal, B is taken initially at time zero.
  • The mole at equilibrium concentration D will be double A to Equilibrium P.
  • Equilibrium constant from A to you will be zero.
  • The concentration of D is double that of A, with x/v being double.
  • Concentration of reactant below product is squared, leading to a value of 3/2.
  • The value of x is 2/3, with the concentration of B being x/√2.
  • The new concentration of S is double the old one, leading to a new concentration of B as 216x cube.
  • The concentration of B and C is calculated to be 20016x cube.
  • The equilibrium constant remains constant, with the concentration of O2 being 4 * 10-2.

02:28:21

"Equilibrium Constants: Delta H, Delta G, Alpha"

  • Taking natural logs on both sides reveals the relationship between the variables.
  • The negative slope indicates a positive reaction.
  • Delta H must be negative for a positive outcome.
  • A break is given before delving into the topic of degree of dissociation.
  • The degree of dissociation, denoted by alpha, is calculated using a specific formula.
  • The observed molar mass at equilibrium mixture is crucial for calculations.
  • The formula for calculating the degree of dissociation involves observed vapor density.
  • The relationship between delta G and delta Ji is explored in the context of free energy changes.
  • The process of finding equilibrium constants involves determining partial pressures.
  • Understanding homogeneous and heterogeneous equilibriums is essential for grasping the concepts discussed.

03:10:15

Equilibrium Constants: Calculations and Shifts

  • The text discusses solving a common problem related to equilibrium constants, emphasizing the importance of not wasting time on derivations.
  • It mentions calculating the partial pressure of a substance 'c' to determine the pressure of 'b'.
  • The text highlights the need to find the total pressure inside a container by adding the pressures of all gases present.
  • It explains a formula to calculate the equilibrium constant of a substance 'p2' divided by the equilibrium constant of both substances.
  • The text delves into the concept of irreversible reactions and their impact on equilibrium.
  • It discusses the significance of concentration changes in reactants and products in affecting equilibrium.
  • The text elaborates on the effect of temperature on endothermic reactions, emphasizing that increasing temperature shifts equilibrium towards heat absorption.
  • It explains how increasing pressure or decreasing volume affects equilibrium, with a focus on the shift based on gaseous moles.
  • The text touches on the importance of understanding the impact of pressure changes on equilibrium, particularly in relation to gaseous moles.
  • It concludes by discussing the consequences of not studying consistently and the importance of maintaining equilibrium in various reactions.

03:29:26

"Pressure's Impact on Equilibrium and Density"

  • Pressure affects the equilibrium position in a reaction; increasing pressure shifts the equilibrium towards the side with fewer gaseous moles.
  • To maximize product yield, keep pressure low to push the equilibrium towards the forward direction.
  • The addition of an inert gas at constant volume does not impact equilibrium, but at constant pressure, increasing volume shifts the equilibrium towards the side with more gaseous moles.
  • Catalysts can be positive or negative; positive catalysts speed up equilibrium attainment, while negative catalysts delay it by increasing activation energy.
  • Temperature influences equilibrium; lower temperatures favor the backward reaction, while higher temperatures favor the forward reaction.
  • Equilibrium remains unaffected by changes in volume or the addition of inert gases at constant volume or pressure.
  • Boylik refers to the temperature at which the vapor pressure of a liquid equals the external pressure, affecting the boiling point.
  • Melting point is influenced by pressure; decreasing volume increases density, as seen in the example of diamond melting.
  • Experimentation with diamond or ice can demonstrate the change in volume upon melting, showcasing the impact of pressure on density.
  • Squats, like quartz, exhibit a decrease in melting point with increasing pressure, leading to an increase in density.

03:48:18

Advancements in Watch Needle Materials and Transformations

  • The needle in a watch is typically made of cords, but with technological advancements, other materials are now used.
  • Increasing volume during melting or elop transformation leads to a decrease in density.
  • When pressure is applied, the melting point decreases, causing water to turn into ice.
  • Reactants with more free energy than products result in a negative Delta G, indicating a spontaneous reaction.
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