Thermodynamics

Capacity factors Depend on the amount of matter present in terms of mass They are equal to the sum of the parts/ additive EX: total volume/total energy of a system

Defines state of a system Properties are interrelated Does not depend on path taken Temperature, pressure, volume, internal energy, enthalpy, entropy

Such as heat (Q) and work (W). Path dependent properties I exact differentials

Intensity factor do not depend on the quantity of material present I.e. Temperature, viscosity, molar volume, density, pressure, refractive index At equilibrium they are the same for every pet of the system

Equation that relates the thermodynamic properties of a system in a state of equilibrium Simplest: PV = nRT

Thermal equilibrium Mechanical equilibrium Chemical equilibrium

The chemical composition of the system does not vary

The pressure is the same everywhere in the system

Occurring at constant pressure Constant P

Occurring at constant volume Constant V

Occurring at constant temperature Constant T

Occurring with no exchange of heat between the system and its surroundings Q = 0

Initial state = final state

Is enclosed by an adiabatic boundary = temperature is independent of its surroundings Never achieves thermal equilibrium with its surroundings I.e. Flow of heat through the boundary = 0

Composed of gases in random motion Collision are perfectly elastic Molecules don’t attract each other U depend only on T and # of molecules

Sum of the energies of the sons Titus the molecules

((P+an^2)/V^2) (V-nb) = nRT a = constant for force of interactions b/w gas particles b = constant for excluded volume

Delta U = Q + W

W = -Pext (Vf-Vi) Involves the movement of matter W = PdV for reversible processes

Is thermal energy that flows from a hot body to a cold one Stored as kinetic and potential energy

Q = (+)

Q = (-)

W = (+)

W = (-)