Thermodynamic Properties Flashcards

These flashcards cover fundamental thermodynamic properties, including definitions of absolute and specific quantities, intensive and extensive properties, states of matter, and enthalpies of phase transitions.

Pressure

A thermodynamic property represented by the symbol $P$ and measured in units of Pascals ($Pa$) or $N/m^2$.

Temperature

A thermodynamic property represented by the symbol $T$ and measured in units of Kelvins ($K$) or degrees Celsius (${}^\text{C}$).

Absolute quantity

A physical quantity that is not relative or dependent on any other factors, such as mass, energy, volume, gravity, and weight or force.

Specific quantity

A physical quantity that is normalized "per unit" of something, such as energy per unit mass.

Specific volume

The volume per unit mass of a substance, which is the reciprocal of density.

Specific gravity

The relative density of a substance with respect to water (density per water density).

Specific mass

Also known as volume-specific mass, it refers to the mass per unit volume.

Specific weight

The weight per unit volume of a substance.

Intensive property or value

A local physical property of a system that does not depend on the system size or the amount of material in the system, such as temperature, density, and viscosity.

Extensive property or value

An additive property for subsystems that increases and decreases as the systems grow larger and smaller, respectively, such as mass, volume, and energy.

Solid state

A state of matter that maintains a fixed volume and shape, with component particles (atoms, molecules, or ions) close together and fixed into place.

Liquid state

A state of matter that maintains a fixed volume but has a variable shape that adapts to its container, with particles that are close together but move freely.

Gaseous state

A state of matter that has both variable volume and shape, adapting both to fit its container, with particles that are neither close together nor fixed in place.

Enthalpy of Fusion

Also known as latent heat of fusion, it is the change in enthalpy resulting from providing energy to a specific quantity of a substance to change its state from solid to liquid at constant pressure.

Enthalpy

The total energy stored in a body or system.

Heat of Solidification

The energy change when a substance changes from liquid to solid, which is equal and opposite to the heat of fusion.

Specific heat of fusion

The heat of fusion referred to a unit of mass.

Heat of fusion of water

The energy value of $79.72 \text{ cal/g}$ or $333.55 \text{ J/g}$ required to change ice to liquid.

Enthalpy of Evaporation

Also known as latent heat of evaporation or vaporization, it is the amount of energy (enthalpy) that must be added to a liquid substance to transform a quantity of it into a gas.

Enthalpy of condensation

The energy change equal to the enthalpy of vaporization but with the opposite sign, where heat is released by the substance.

Enthalpy of vaporization of water

The energy value of $40.660 \text{ J mol}^{-1}$ or $2257 \text{ J g}^{-1}$ ($40.65 \text{ kJ/mol}$) required to transform water into gas.

Fluid

A phase of matter including liquids, gases, and plasmas that continually deforms (flows) under an applied shear stress or external force and cannot resist any shear force.

Cavitation

A phenomenon in liquids caused when their tensile strengths are exceeded.

Plasticity

The characteristic of solids where they require a certain initial stress before they deform.