Equilibrium

Equilibrium involves dynamic reactions that can go forward and backward, achieving a balance between reactants and products in a closed system, guided by Le Chatelier's principle.

Dynamic Equilibrium And Le Chatelier's Principle

This section covers the concepts of dynamic equilibrium and Le Chatelier's Principle, explaining how reversible reactions achieve equilibrium and how changes in concentration, pressure, and temperature affect this state.

Key Characteristics Of Dynamic Equilibrium

Dynamic equilibrium refers to the state where the rates of forward and reverse reactions are equal in a closed system, resulting in constant macroscopic properties.

Le Chatelier's Principle

Le Chatelier's Principle describes how a system at equilibrium responds to changes in concentration, pressure, and temperature, aiming to counteract disturbances.

Effect Of Concentration Changes

This section outlines how changes in concentration affect dynamic equilibrium in reversible chemical reactions.

Effect Of Pressure Changes (For Reactions Involving Gases)

This section describes how changes in pressure impact the position of equilibrium in gaseous reactions, aligning with Le Chatelier's Principle.

Effect Of Temperature Changes

Temperature changes significantly affect both the position of chemical equilibrium and the value of the equilibrium constant.

Effect Of A Catalyst

A catalyst increases the rate of a chemical reaction without altering the position of equilibrium, facilitating the system to reach equilibrium faster.

Equilibrium Constant (Kc And Kp)

This section discusses the equilibrium constants Kc and Kp, which quantitatively express the ratios of concentrations and partial pressures of products and reactants at equilibrium.

Important Considerations For Kc

This section discusses key factors affecting the equilibrium constant (Kc) of a chemical reaction, including temperature dependence, the inclusion of phases, units of Kc, and the significance of Kc values in understanding reaction dynamics.

Equilibrium Constant In Terms Of Partial Pressures (Kp)

The equilibrium constant in terms of partial pressures (Kp) is a crucial concept for quantifying the relationship between the concentrations of reactants and products in a gaseous chemical equilibrium.

Relationship Between Kc And Kp

This section explains the relationship between the equilibrium constants Kc and Kp, highlighting their definitions and how they are affected by temperature and the change in moles of gas during a reaction.

Calculations Involving Equilibrium Constants

This section focuses on how to calculate equilibrium constants (K) from equilibrium concentrations and how to predict equilibrium concentrations using ICE tables.

Scenario 1: Calculating The Value Of K From Equilibrium Concentrations/partial Pressures

This section covers the calculation of the equilibrium constant (K) based on the equilibrium concentrations or partial pressures of reactants and products.

Scenario 2: Calculating Equilibrium Concentrations/partial Pressures From Initial Conditions And K (Ice Tables)

This section discusses how to calculate equilibrium concentrations or partial pressures using initial conditions and the equilibrium constant (K) through the application of ICE tables.

Approximation Method

The Approximation Method simplifies equilibrium calculations for reactions with small K values.

Hl: Relationship Between Δg And K

This section discusses the relationship between the Gibbs free energy change (ΔG) and the equilibrium constant (K), illustrating how they dictate the spontaneity and extent of chemical reactions.

Standard Gibbs Free Energy Change (Δg°)

This section explains the relationship between Gibbs free energy change (ΔG°) and the equilibrium constant (K) for chemical reactions, helping to determine spontaneity and thermodynamic favorability.

The Fundamental Relationship

This section discusses the relationship between standard Gibbs free energy change (ΔG°) and the equilibrium constant (K), highlighting its significance in predicting the spontaneity of reactions.

Understanding The Relationship

This section explores the crucial link between Gibbs free energy change (ΔG) and equilibrium constant (K), underscoring how they jointly inform the spontaneity and direction of reactions.

Temperature Dependence Of K

This section discusses how the equilibrium constant (K) for a chemical reaction varies with changes in temperature, emphasizing the underlying thermodynamic principles.

Calculating K From Δg° Or Vice Versa

This section explains the relationship between Gibbs free energy change (ΔG°) and the equilibrium constant (K), providing a method to calculate one from the other at a specific temperature.