Thermodynamics Flashcards
change in temperature of most solids (and liquids) results in change in legth
thermal expansion
thermal expansion of solid
∆L = αL∆T
where:
L = initial length
α = coefficient of linear expansion (K^-1) = 1/3 β
thermal expansion of liquid
∆V = βV∆T
where:
V = initial volume
β = coefficient of volumetric expansion (K^-1) = 3 α
non-state functions
work and heat; describe path taken from one state to another
system not capable of exchanging energy or matter with surroundings
isolated system
system capable of exchanging energy but not matter with surroundings
closed system
system capable of exchanging energy or matter with surroundings
open system
amount of heat required to raise 1 g of water 1 °C
calorie (little c)
amount of heat required to raise 1 kg of water 1 °C
Calorie (big C)
1 C = ___ c = ___ J
1 c = ___ J
1 C = 1000 c = 4184 J
1 c = 4.184 J
direct transfer of energy from molecule to molecule through molecular collisions
conduction
transfer of heat by physical motion of fluid over a material
convection
transfer of energy by electromagnetic waves
radiation
change in internal energy (U)
∆U = q - w
specific heat (c)
q = mc∆T
units of c = 1 cal/gK = 4.184 J/gK
heat of transformation/latent heat (L)
q = mL
solid to liquid
fusion or melting
liquid to solid
freezing or solidification
liquid to gas
boiling, evaporation, or vaporization
gas to liquid
condensation
solid to gas
sublimation
gas to solid
deposition
isothermal process
constant temp, ∆U = 0 –> q = w
adiabatic process
no heat exchange, q = 0 –> ∆U = -w
isobaric process
constant pressure
isochoric process
constant volume (isovolumetric), w = 0 –> ∆U = q
entropy (S)
∆S = q(rev) / T
unit of S = J/mol*K
objects are in thermal equilibrium when they are at the same temperature
zeroeth law of thermodynamics
the total energy in the universe can never increase or decrease
first law of thermodynamics
in a closed system, energy will spontaneously and irreversibly go from being localized to being spread out
second law of thermodynamics
