Dynamic and Static Equilibrium in Chemical Reactions

Dynamic Equilibrium

State where forward and reverse reactions occur simultaneously.

Reversible Reaction

Reaction that can proceed in both forward and reverse directions.

Equilibrium

Condition where reactant and product concentrations remain constant.

Yield

Extent of conversion of reactants into products.

Closed System

System where reactants and products cannot escape.

Haber Process

Production of ammonia from nitrogen and hydrogen gases.

Collision Theory

Theory explaining reaction rates based on particle collisions.

Forward Reaction

Process where reactants form products.

Reverse Reaction

Process where products reform reactants.

Equilibrium Mixture

Combination of reactants and products at equilibrium.

Dynamic State

Equilibrium characterized by ongoing reactions.

Dinitrogen Tetroxide

Compound that decomposes to nitrogen dioxide.

Nitrogen Dioxide

Dark brown gas formed from dinitrogen tetroxide.

Extent of Reaction

Measure of product formation at equilibrium.

Strong Acid

Acid that completely dissociates in solution.

Weak Acid

Acid that partially dissociates in solution.

Hydrochloric Acid

Strong acid that fully dissociates in water.

Ethanoic Acid

Weak acid that partially dissociates in water.

Conductivity

Ability of a solution to conduct electricity.

Dissociation

Process of breaking down into ions in solution.

Equilibrium Constant

Ratio of product concentrations to reactant concentrations.

Reaction Rate

Speed at which reactants convert to products.

Molecular Level

Scale at which individual particles interact.

Color Change

Observable change indicating reaction progress.

Concentration vs. Time Graph

Visual representation of concentration changes over time.

Equilibrium System

System where reactants and products are balanced.

Chemical Reaction

Process where substances transform into different substances.

Ammonia Production

Formation of NH3 from N2 and H2.

Reaction Vessel

Container where chemical reactions occur.

Rate of Reaction

Change in concentration over time for reactants/products.

Reversible Reactions

Reactions that can proceed in both forward and reverse.

Static Equilibrium

No movement; rates of reactions are almost zero.

Activation Energy

Minimum energy required for a chemical reaction.

Non-Equilibrium Systems

Systems that do not reach equilibrium state.

Combustion Reactions

Irreversible exothermic reactions releasing energy.

Photosynthesis

Endothermic process converting CO2 and H2O into glucose.

Entropy

Measure of disorder or randomness in a system.

Gibbs Free Energy

Determines spontaneity of reactions; ΔG = ΔH - TΔS.

ΔH

Change in enthalpy; heat content of a system.

ΔS

Change in entropy; measure of disorder change.

Spontaneous Reaction

Occurs without continuous energy supply; ΔG is negative.

Non-Spontaneous Reaction

Requires external energy to proceed; ΔG is positive.

Chemical Energy

Energy stored in chemical bonds of molecules.

Endothermic Reaction

Absorbs heat; ΔH is positive.

Exothermic Reaction

Releases heat; ΔH is negative.

Activation Energy Barrier

Energy threshold for reactants to form products.

Equilibrium Position

Concentration ratio of products to reactants at equilibrium.

Chemical Kinetics

Study of reaction rates and mechanisms.

Thermodynamics

Study of energy transformations in chemical processes.

Second Law of Thermodynamics

Entropy of the universe always increases.

Coupled Reactions

Spontaneous reactions drive non-spontaneous reactions.

Carbon Dioxide

Gas produced in combustion and consumed in photosynthesis.

Glucose

Product of photosynthesis; energy source for plants.

ΔSsurroundings

Entropy change of the surroundings during a reaction.

Energy Transfer

Movement of energy from one system to another.