Thermodynamics

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Key Terms

System, Surrounding, boundary, State function, path function, work, internal energy, enthalpy, bomb calorimeter, Temperature conversion

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Terms and Definitions

State-function – A property whose value does not depend on the path taken to reach that specific value.
Heat-transfer – The movement of heat energy from one object to another.
Work-done – Energy transferred when a force moves an object.
First-law – A principle stating that energy cannot be created or destroyed, only transformed.
Second-law – A law stating that total entropy of an isolated system can only increase over time.
Open-system – A system that exchanges both energy and matter with its surroundings.
Closed-system – A system that exchanges energy but not matter with its surroundings.
Isolated-system – A system that does not exchange energy or matter with its surroundings.
Standard-enthalpy – The change in enthalpy when one mole of substance is formed under standard conditions.
Gibbs-free energy – A thermodynamic quantity that measures the useful work obtainable from a system.
Spontaneous-process – A process that occurs without needing to be driven by an external energy source.
Non-spontaneous – A process that requires external energy to proceed.
Equilibrium-state -A condition in which all competing influences are balanced in a system.
Reaction-enthalpy – The change in enthalpy when a reaction occurs at constant pressure.
System-boundary – The interface separating a system from its surroundings.
Path-function – A property that depends on the route taken between initial and final states.
Internal-energy – The total energy contained within a system.
Entropy-change – The change in entropy when a process occurs.
Reversible-process – A process that can be reversed without any net change in the system and surroundings.
Irreversible-process – A process that cannot return the system to its original state.
Heat-capacity – The amount of heat needed to increase the temperature of an object by a certain amount.
Molar-enthalpy – Enthalpy per mole of a substance.
Specific-heat – The heat required to raise the temperature of the unit mass of a substance by one degree.
Enthalpy-change – The total heat content change in a system at constant pressure.
Energy-conservation – The principle that the total energy of an isolated system remains constant.
Chemical-potential – The potential energy of molecules which drives chemical reactions.
Standard-state – A reference state for a substance used to calculate its properties under different conditions.
Partial-pressure – The pressure exerted by a single component in a mixture of gases.
Thermal-equilibrium – A condition where all parts of a system are at the same temperature.
Heat-of-reaction – The change in heat during a chemical reaction at constant pressure.
Equilibrium-constant – A number that expresses the relationship between products and reactants at equilibrium.