Formula And Laws For Physics Ii Test 2 Fluids Thermodynacis

Front 1

density of a fluid at rest

Back 1

p2 = p1 + (rho)g(y1-yo0)

Front 2

gauge pressure

Back 2

Pabs = Pgauge + P0

Front 3

pressure

Back 3

p=F/A

Front 4

density

Back 4

(rho)=m/V

Front 5

Pascal's Principle

Back 5

F1/A1=F2/A2

Front 6

Archemide's Principles (buoyancy)

Back 6

Fb=(rho)Vg

Front 7

equation of continuity/volumetric flow rate

Back 7

A1v1=A2v2

Front 8

Bernoulli's equation

Back 8

p1+.5(rho)v1^2+(rho)gy1=p2+.5(rho)v2^2+(rho)gy2

Front 9

ideal gas law

Back 9

pV=nRT

Front 10

ideal gas law 2

Back 10

pV=NKbT

Front 11

number of moles

Back 11

m/M=N/Na

Front 12

0th law of thermodynamics

Back 12

2 connected objects at thermal equilibrium with each other are at same temperature

Front 13

Kelivin to Celcius

Back 13

Tc=T-273K

Front 14

celcius to farenheit

Back 14

Tf=9/5Tc+32f

Front 15

change in length

Back 15

(alpha)Li(delta)T

Front 16

change in area

Back 16

(gamma)Ai(delta)T

Front 17

change in volume

Back 17

(beta)Vi(delta)T

Front 18

molecular interpretation of pressure

Back 18

p=(2/3)(N/V)(.5mvave^2)

Front 19

molecular interpretation of temperature

Back 19

(3/2)KbT=.5mvave^2

Front 20

Total kinetic energy of N molecules

Back 20

KEtot=N(.5mvave^2)=(3/2)NKbT=(3/2)nRT

Front 21

equipartition theorem

Back 21

each degree of freedom contributes .5KbT of energy

Front 22

internal energy of monatomic gas

Back 22

KE=(3/2)nRT

Front 23

.5KbT of monatomic gas

Back 23

.5mvavex^2=.5mvavey^2=.5mvavez^2

Front 24

most probable velocity of molecule of monatomic gas

Back 24

vmp=sqrt(2KbT/m)

Front 25

average velocity of molecule of monatomic gas

Back 25

vave=sqrt(8KbT/(pi)m)

Front 26

change in energy from temperature change

Back 26

Q=mc(delta)T

Front 27

change in energy from phase change

Back 27

+-mL(f or v)

Front 28

molar equation for change in energy from temperature change at constant volume

Back 28

Q=nCv(delta)T

Front 29

molar equation for change in energy from temperature change at constant pressure

Back 29

Q=nCp(delta)T

Front 30

(delta)Eint or (delta)U for all gases

Back 30

nCv(delta)T

Front 31

R for all gases

Back 31

R=Cp-Cv

Front 32

gamma for all gases

Back 32

(gamma)=Cp/Cv

Front 33

Cv for monatomic gases

Back 33

Cv=(3/2)R

Front 34

Cp for monatomic gases

Back 34

Cp=(5/2)R

Front 35

gamma for monatomic gases

Back 35

(gamma)=5/3

Front 36

total number of degrees of freedom for diatomic gas

Back 36

7

Front 37

constants in adiabatic process

Back 37

PV^(gamma)
TV^((gamma)-1)

Front 38

work in adiabatic process

Back 38

W=(PiVi-PfVf)/((gamma)-1)=nCv(Ti-Tf)

Front 39

(delta)Eint or (delta)U

Back 39

(delta)Eint=Q-W

Front 40

process in which there is no heat exchange

Back 40

adiabatic

Front 41

process in which there is no change in pressure

Back 41

isobaric

Front 42

process in which there is no change in volume

Back 42

isochoric / isovolumetric

Front 43

process in which there is no change in temperature

Back 43

isothermal

Front 44

2nd law of thermodynamics (form 1)

Back 44

there is no perfect engine

Front 45

COP(heat)

Back 45

|Qh|/W=|Qh|/(|Qh|-|Qc|)=COP(heat)

Front 46

efficiency

Back 46

e=W/|Qh|=(|Qh|-|Qc|)/|Qh|

Front 47

2nd law of thermodynamics (form 2)

Back 47

there is no perfect refrigerator

Front 48

COP(cool)

Back 48

|Qc|/W=|Qc|/(|Qh|-|Qc|)

Front 49

2nd law of thermodynamics (form 3)

Back 49

in any thermodynamic process that proceeds from one equilibrium state to another, the entropy of the system and environment either remains unchanged or increases

Front 50

change in entropy of reversible process

Back 50

(delta)S=Sf-Si=(integral of)dQr/T

Front 51

change in entropy of an irreversible process

Back 51

(delta)S=Sf-Si=(integral of)dQ/T