Equilibrium Constants and Le Châtelier's Principle

Equilibrium Constant

Ratio of product concentrations to reactant concentrations.

Reciprocal Constant

Reverse reaction's constant is the reciprocal of forward.

Multiplying Reactions

Constant raised to the power of the multiplier.

Net Reaction Constant

Product of constants from individual reaction steps.

Equilibrium Concentration

Concentration of substances at equilibrium state.

Kc Calculation

Kc = [HI]^2 / ([H2][I2]).

Initial Concentrations

Starting concentrations before equilibrium is reached.

Le Châtelier's Principle

System shifts to counteract disturbances in equilibrium.

Reactant Addition Effect

Increasing reactant concentration shifts equilibrium right.

Product Removal Effect

Removing product shifts equilibrium to produce more.

Haber Process

Conversion of nitrogen and hydrogen to ammonia.

Ammonia Significance

Ammonia is crucial for agricultural fertilizers.

Pressure Change Effect

Increasing pressure shifts equilibrium to fewer gas moles.

Exothermic Reaction

Releases heat; shifts left with temperature decrease.

Catalyst Role

Increases reaction rates without altering equilibrium.

Gas Volume Principle

Equal moles of gas occupy equal volumes.

Equilibrium Shift Prediction

Shift direction predicted by changes in conditions.

Concentration Decrease Effect

Removing a reactant shifts equilibrium to the left.

Heat as Product

In exothermic reactions, heat is a product.

Equilibrium Composition

Final concentrations of reactants and products at equilibrium.

Dynamic Equilibrium

Rates of forward and reverse reactions are equal.

Concentration Change

Adding or removing substances alters equilibrium position.

Volume Decrease Effect

Decreasing volume increases pressure, shifts equilibrium.

Equilibrium Constant Units

Units depend on reaction stoichiometry and concentrations.

Equilibrium Expression

Mathematical representation of equilibrium constant.

Reaction Quotient (Q)

Calculates current state compared to equilibrium state.

Equilibrium Shift Factors

Temperature, pressure, and concentration affect equilibrium.

Mole Ratio

Stoichiometric coefficients define mole relationships in reactions.

Equilibrium System

Closed system where reactants and products coexist.

Temperature Effect on Equilibrium

Temperature changes affect exothermic and endothermic reactions.

Equilibrium Constant Change

Kc varies with temperature but not pressure.

Chemical Equilibrium

State where reactants and products remain constant.

Reaction Rate

Speed at which reactants convert to products.

Equilibrium Dynamics

Constant changes in concentrations while achieving balance.