Chemistry for Engineers - Equilibrium and Energetics

A set of vocabulary flashcards summarizing key concepts from the 'Chemistry for Engineers' lecture on equilibrium, chemical energetics, and bonding.

Equilibrium

A state in which a chemical or physical system remains unchanged over time, representing a dynamic balance.

Chemical Equilibrium

Applies to reversible reactions where concentrations of reactants and products remain constant.

Le Chatelier’s Principle

States that a system at equilibrium will shift its position to counteract changes in conditions.

Equilibrium Constant (K)

A ratio that expresses the concentrations of products to reactants at equilibrium under specific conditions.

Reversible Reaction

A reaction that can proceed in both forward and reverse directions.

Phase Equilibrium

Occurs during transitions between solid, liquid, and gas phases where amounts coexist without net change.

Catalyst

A substance that increases the rate of a reaction without affecting the position of equilibrium.

Hess’s Law

States that the overall enthalpy change of a reaction is independent of the pathway taken.

Enthalpy (H)

A thermodynamic property that measures the heat content of a system.

Bond Energy

The energy required to break a chemical bond.

Ksp (Solubility Product Constant)

A measure of the solubility of a sparingly soluble compound in water.

Endothermic Reaction

A reaction that absorbs heat, resulting in a positive enthalpy change (∆H > 0).

Exothermic Reaction

A reaction that releases heat, resulting in a negative enthalpy change (∆H < 0).

Enthalpy Change (∆H)

The heat energy exchanged between a system and its surroundings during a chemical reaction.

Bond Enthalpy

The enthalpy change associated with breaking a specific bond in one mole of gaseous substance.