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1
Q

what is an operational definition of temperature

A

The temperature of a substance is a measure of the mean

translational kinetic energy associated with the disordered microscopic motion of its constituent atoms or molecules.

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2
Q

direction of heat flow

A

Heat flows from a region of higher temperature toward a region of lower temperature.

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3
Q

things needed to make a theromometer

A

a system with a suitable thermometric property,

an easily duplicated method of construction

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4
Q

what does a useful thermometer have

A

reproducible readings, small heat capacity(so it doesnt change the properties of the system), a wide operating range

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5
Q

thermometric property

A

is any physical property that changes measurably with temperature

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6
Q

Good Thermometric Property

A

independent of the properties and sample-dependence of specific substance

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7
Q

pressure temp law

A

The pressure p of a fixed mass of gas at low density in a constant volume is proportional to the absolute temperature, T

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8
Q

Constant-Volume Gas Thermometer operation

A

Allow gas and system to reach thermal
equilibrium, Adjust height of mercury reservoir to
bring meniscus to the constant volume
reference mark, Measure the height h and hence determine the pressure p, Use T = ap, where a is a constant for the thermometer to determine the temperature T

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9
Q

Constant-Volume Gas Thermometer used to compare temp of systems

A

T1=ap1 T2=ap2 therfore T1/T2=p1/p2

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10
Q

Kelvin scale

A

Based on properties of an ideal gas and the 2nd Law of
Thermodynamics, Requires only a single fixed point defined as T triple point= 273.16K, The value for
T triple point is defined so that (T melting point)–(Tboiling point)= 100K

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11
Q

Celcius temperature scale

A

Uses pure water at 101 kPa to determine two fixed points, which are defined as being 100 degrees apart (hence
centigrade)

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12
Q

thermodynamic temperature scale

A

one that does not depend on the properties of the substances that are used to measure temperature

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13
Q

why is kelvin thermodynamic

A

because it is based on: Equation of state of an ideal gas, Properties of a reversible heat engine

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14
Q

Calibration of the CV Gas Thermometer

A

The triple-point of pure water gives a very reproducible temperature reference, Error bounds of +0.0μK/ –150μK are achievable. This allows determination of the calibration constant a for a CV gas
thermometer. For low pressures results become independent of the gas used.

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15
Q

how are thermodynamic properties of a system determined

A

by its thermodynamic state

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16
Q

how is the thermodynamic state of a system specified

A

by values of a suitable set of parameters known as

state variables

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17
Q

State variables

A

density ρ, enthalpy H, entropy S, internal energy

U, mass M, number of moles n, chemical potential μ,pressure p, temperature T, volume V

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18
Q

Equation of State definition

A

a mathematical relationship between state variables

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19
Q

An equation of state properties

A

exists for every thermodynamic system, cannot be determined using thermodynamics, can be determined from experiments or a molecular theory, for a closed system, relates T to two other variables

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20
Q

The equation of state of an ideal gas

A

pV=nRT, useful approximation for real gases at low

p or high T

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21
Q

Path-Independence of State

A

Independent of the path (sequence) of state-variable values used to make the change

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22
Q

The P-V-T Surface

A

The state variables p, V, T, n are the coordinates in a 4-space, The equation of state defines surfaces in this space

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23
Q

Isotherms

A

p vs V at constant temperature

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24
Q

Isobars

A

V vs T at constant pressure

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25
Q

Isochors

A

p vs T at constant volume

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26
Q

critical temperature

A

above this the gas cant be liqified by preassure alone

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27
Q

Van der Waals Equation of State

A

(p+an^2/V^2)(V-nb)=nRT

a and b are empirical constants that differ for each gas

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28
Q

info about Van der Waals Equation of State

A

takes into account : molecular volume which is nbso the volume available for the molecules to move in is (V–nb),Intermolecular attraction is represented by an^2/V^2.This decreases the pressure at high densities

29
Q

Virial Equation of State

A

pV/nRT=1+……Bn(n/v)^n

Bn are the virial coefficients. These are specific to each gas and are functions of T

30
Q

Virial Equation of State info

A

uses a power-series expansion, reduces to the ideal gas equation of state at low densities, can be derived using
statistical mechanics, is valid for any isotropic substance if enough terms are used.

31
Q

Equation of State for a Simple Solid

A

V =V0[1+β(T−T0)−kT(p−p0)]
kT=−ΔV/V0Δp is the isothermal compressibility
β=ΔV/V0ΔT is the isobaric volumetric expansivity

32
Q

Heat is

A

measure of the energy transferred between two systems as a result of a temperature difference,

33
Q

specific heat capacity equation

A

ΔQ=cMΔT

34
Q

Specific heat capacity holding preassure constant

A

c=1/M(δQ/dT)

35
Q

Specific heat capacity holding volume constant

A

c=1/M(δQ/dT)

36
Q

three mechanisms that transfer heat between systems

A

Conduction, Convection, Radiation

37
Q

importance of heat transfer mechanisms depends on

A

nature of the systems, geometry of the systems, temperature regime involved

38
Q

Conduction is

A

the transfer of heat through a medium that is stationary on a macroscopic scale

39
Q

thermal resistance equation

A

R=L/κA k=thermal conductivity L=legnth A=cross sectional area

40
Q

charge thermal equivalent

A

heat

41
Q

current thermal equivalent

A

heat flux

42
Q

capacitance thermal equivalent

A

heat capacity

43
Q

pd thermal equivalent

A

temp

44
Q

reistance thermal equivalent

A

thermal resistance

45
Q

Convection

A

the transfer of heat via the movement of a medium on a macroscopic scale important in fluids

46
Q

Convection forced

A

externally driven flow

47
Q

Convection free

A

thermally induced density gradients drive the flow

48
Q

Radiation is

A

the transfer of heat via electromagnetic waves, No medium is required,

49
Q

Stefan-Boltzmann law

A

P=εσAT^4 for p net T^4-Tenv^4

50
Q

Kinetic Theory of Gases assumptions

A

A container with volume V contains a very large number N of identical spherical molecules, each with mass m
The molecular radius is small compared with the average distance between molecules and the size of the container
The molecules are in constant rapid random motion and obey Newton’s laws
There is no force acting between molecules except during
collisions.
The molecules collide with each other and with the
walls of the container. All collisions are perfectly elastic
The container walls are perfectly rigid and infinitely massive
The gas is in equilibrium

51
Q

Collision Frequency of molecules with wall

A

(N/2V)A∣v_x∣dt

52
Q

The gas is isotropic so

A

v^2x=v^2y=v^2z=(1/3)v^2total

53
Q

force exerted by gas

A

Fx=momentum change x arrival rate =2mv (N/2V)A∣v_x∣

54
Q

pressure equation

A

force/area = 1/3Nmv^2

55
Q

Microscopic Interpretation of Temperature

A

mean translational kinetic energy

per molecule

56
Q

Internal Energy of the Ideal Gas assumptions

A

No intermolecular forces
No rotational kinetic energy
No vibrational kinetic energy

57
Q

Internal Energy of the Ideal Gas equations

A

3/2NkT=3/2NnRT

58
Q

The heat capacity of n moles of ideal gas

A

3/2nRT

59
Q

velocity density

function

A

f(v)=Aexp(−Bv^2) v=sqrt(ln(v)/2) at half height

A=sqrt(B/pi)

60
Q

speeds of molecules

A

v most probable < v average < v rms

61
Q

Ideal gas model does not describe

A 
thermal conductivity
electrical resistivity
viscosity
diffusion
because these depend on the frequency of collisions between molecules
62
Q

collision rate of one molecule with other stationary molecules

A

(N/V)4πr^2⟨v⟩

63
Q

collision rate of one molecule with other moving molecules

A

(N/V)4√2πr2⟨v⟩

64
Q

mean free path proportionalities

A

λ∝T. λ∝1/p

65
Q

viscosity

A

momentum transfer

66
Q

thermal conductivity

A

energy transfer

67
Q

coefficient of diffusion

A

mass transfer

68
Q

Thermal Conductivity proportionalities

A

independent of density κ∝(1/r^2)sqrt(T/m)

properties of matter (1 decks)

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