Lecture 2 - Laws of Thermodynamics (DOBSON) Flashcards
What is the zeroth law of thermodynamics?
If two systems are (individually) in equilibrium with a thrid system, they are also in thermal equilibrium with each other. DRAW DIAGRAM. Systems in thermal equilibrium do not exchange heat. The temps are equal for all systems in thermal equilibrium.
What is the first law of thermodynamics?
(Expresses the principle of conservation of energy). Energy can be transformed (changed from one form to another) but cannot be created or destroyed. Formulated by stating that the change in internal energy of a system (U) is equal to the amount of heat applied to the system (Q), minus the amount of work performed by the system on its surroundings (W). dU = dQ - dW
What is the second law of thermodynamics?
After a certain amount of time, isolated physical systems reach equilibrium. In any cyclic process the entropy will either increase or remain the same. dS >/= 0
What is the third law of thermodynamics?
This states that the entropy of a perfect crystal approaches zero as the absolute temp approaches zero. In doing so it provides an absolute reference point for the determination of entropy. S=0 when T=0
How can heat transfer in fluids be understood?
By considering the kinetic theory of gases.
What assumptions does the kinetic theory of gases rely on?
- The gas consists of very small particles. This small size is such that the total volume of individual gas molecules added up is negligible compared to the volume of the container.
- These particles have the same mass.
- The number of molecules is so large that statistical treatment can be applied.
- These molecules are in constant, random & rapid motion.
- The rapidly moving particles constantly collide among themselves and with the walls of the container. All of these collisions are perfectly elastic.
- Except during collisions, the interactions among molecules are negligible.
- The average kinetic energy of the gas particles depends only on the temp. of the system.
What is the expression to describe the kinetic energy of a single particle?
(1/2).m.(v_rms^(2)) = (3/2).K_b.T
What happens if there is a spatial variation in temp of the fluid?
This will tend to equilibriate due to successive collisions between the particles. In this way, heat can be conducted through the fluid.
How can particles gain and lose KE?
gain (increase temp) by coming into contact with a hot surface. Lose (decrease temp) by colliding with a cold surface. (in this way gas can transfer heat with a solid surface and heat can be transferred between two solid surfaces via an intermediate fluid.
Will the rate of heat transfer be faster for a hot fluid or a cold fluid?
Faster for a hot fluid because hot particles move faster than cold ones. (hot fluids have higher thermal conductivity)
What is mean free path?
The mean distance that a particle travels before colliding with another particle: l = K_b.T/(sqrt(2).pi.d^(2).p) l=mean free path K_b = Boltzmann's constant T = Temp d = atomic (molecular diameter) p = pressure
How is heat conduction analogous to no. of cars on a motorway?
If an individual particle can travel from one surface to another without any collisions, it will conduct heat very well. However, if we achieve this by decreasing the pressure we also greatly reduce the no. of particles available to conduct the heat.
Can you draw the graph of conductivity vs pressure?
YES OR NO
What does the thermal conductivity of a gas ultimately depend on?
Temp, pressure and amount of energy each particle is capable of carrying (heat capacity).
Equation for calculating the conductivity of an ideal gas?
K = nlambdaCv/3N_a. K=conductivity n = no. of particles per volume v = mean particle speed lambda = mean free path Cv = molar heat capacity N_a = Avogadro's number