Thermodynamics Flashcards
Three types of systems that one measure is constant:
isochoric: no change in volume
isobaric: pressure constant
isothermic: no change in temp
Three types of thermodynamic systems
isolated: no exchange matter or energy
closed: no exchange matter, but energy okay
open: exchange matter and energy
Zeroth law
- transitive prop: everything in contact is going to be in equilibrium
1st law thermo:
energy and matter not created or destroyed:
Delta U = Q - W
Q: heart flow
W: work
2nd law thermo:
What is unit of heat?
What does 1 Cal equal
entropy
- always increasing, precludes perfectly efficient transfer
- net entropy increase of 0
- heat = J
- 1 Cal = 1000 cal = 4184 J = raise 1 kg water 1 C
sign convention of work in regards to a system:
work done on system: system gaining internal energy
- W = pos
work done by system: system losing internal energy
- W = neg
KE ideal gases
- Vrms = square root (3RT/Mm)
KE = 3/2T(Rmparticle/Mm)
Derive the components of Work equation: W = ***
-P*delta V
P = force/Area > F - PA
W = PA(delta)x
Fareneight to Celsius:
F = 9/5C + 32
Linear and volumetric expansion can be simplified as:
Change in temp * constant * length/volume respectively
- volume constant = 3x linear constant
What is the specific heat question?
q = mc delta T
c: specific heat
What is heat of transformation equation?
q = mL
Solid to liquid:
Fusion/melting
- melting point
Liquid to solid:
Freezing
- freezing point
Liquid to gas:
Vaporization/boiling/evaporation
- boiling point
