Gen chem chapter 7

isolated

systems that exchange neither matter nor energy with the environment

closed

systems that exchange energy but not matter with the environment

open

systems that exchange energy and matter with the environment

isothermal

processes that occur at the same temp

adiabatic

processes that exchange no heat with the environment

isobaric

processes that occur at a constant pressure

isovolumetric/isochoric

processes that occur at a constant volume

state functions

describe the physical properties of an equilibrium state. They are pathway independent and include pressure, density, temperature, volume, enthalpy, internal energy, gibbs free energy, and entropy

standard conditions

273, 1atm, and 1M

fusion(melting) and freezing

occur at the boundary between solid and liquid phase

vaporization and condensation

occur at the boundary of liquid and gas phases

sublimation and deposition

occur at the boundary between solid and gas phase

triple point

point where all 3 phases of matter exist in equilibrium

phase diagram

graphs the phases and phase equilibrium as a function of temperature and pressure

temperature

a scaled measure of the average kinetic energy of a substance

heat

transfer of energy that results from differences of temperature between two substances

enthalpy

a measure of the potential energy of a system found in intermolecular attractions and chemical bonds

hess’s law

states that the total change in potential energy of a system is equal to the changes of potential energies of the individual steps of the process

entropy

a measure of the degree to which energy has been spread throughout a system, or between a system and its surroundings (maximized and equilibrium)

Gibbs free energy (G)

derived from both enthalpy and entropy values. The change in this determines a reactions spontaneity(depends on temperature)

spontaneous/formward

ΔG<0

nonspontaneous/reverse

ΔG>0

dynamic equilibrium

ΔG=0