Thermodynamics I Flashcards
What is a system?
- Surrounding- outside the flask
- Boundry - the flask
- System - things within the flask
Isolated syatem
- In a vacum due to no change of energy in
- No mass or heat transer
Closed system
- Mass transfer yes heat transfer no
Open system
- Both mass and heat can be exchanged
Constant volume (Isovolumetric)
- delta U = q
- no work done by the system
- Any energy change is result of heat transfer
Constant Temperature (Isothermal)
- q = w
- No change in internal energy
- Any heat transferred to the system is used to do work
No Heat Transfer (Adiabatic)
- ∆U = w
- Internal energy changes only for work done or received by the system
Dela U = Q - W
Delta U = change in internal energy
Q = Heat added to system
W = Work done by system
1 cal
Heat needed to raise the temperature pf 1g of water by 1 degree at a standard pressure
Enthalphy
- Measure of the energy in a thermodynamic system
- q<0 exothermic
- q>0 endothermic
Second law of thermodynamics
Universe moving towards maxium disorder
S = Kb ln(W)
KB = Boltzmann constant (energy of an individual atom)
W = microstates (ways to arrange particles in a system)
Microstates
- Arangement of particles in space movement diffrent positions increse entropy when open system cased by Increased microstates
Third Law of thermodynamics
At absolute zero (0 K), the entropy of a perfect, crystalline substance is zero
Third Law of thermodynamics
At absolute zero (0 K), the entropy of a perfect, crystalline substance is zero
