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Physics Revision Year 1 > Thermodynamics 1 > Flashcards

Thermodynamics 1 Flashcards

1
Q

Centigrade and Farenheit Scale

A

Tc = 5/9 (Tf - 32)

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2
Q

Gas Thermometers

A

Gas thermometers all agree with each other in the measurement of any temperature as long as the density of the gas is very low.
T = (P/P3)*T3

where
P = observed pressure of gas in the thermometer
P3 = pressure when the thermometer is immersed in a water-ice-vapour bath at its triple point
T3 = 273.15K (the triple point temperature)

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3
Q

Ideal Gas

Equation of State

A

PV = nRT

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4
Q

Universal Gas Constant

A

R = 8.31 J/molK = 0.821 Latm/mol*K

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5
Q

Boltzmann’s Constant

A

k = 1.381x10^-23 J/K

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6
Q

Advogadro’s Number

A

Na = 6.022x10^23

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7
Q

Ideal Gas

Equation for a Fixed Amount of Gas

A

P2V2/T2 = P1V1/T1

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8
Q

Kinetic Theory of Gases

Molecular Interpretation of Temperature

A

The absolute temperature T is a measure of the average molecular translational kinetic energy.

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9
Q

Kinetic Theory of Gases

Equipartition Theorem

A

When a system is in equilibrium, there is an average energy of 1/2 kT per molecule (1/2 RT per mole) associated with each degree of freedom.

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10
Q

Kinetic Theory of Gases

Total Translational Kinetic Energy

A

Ktrans = N(1/2 mv²)av = 3/2 NkT = 3/2 nRT

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11
Q

Kinetic Theory of Gases

RMS Speed of Molecules

A

vrms = √[(v²)av] = √[3kT/m] = √[3RT/M]

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12
Q

Kinetic Theory of Gases

Mean Free Path

A

λ = 1/[√2* nv* d²*π]

nv = number of molecules per unit volume

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13
Q

Maxwell-Boltzmann Speed Distribution

A

f(v) = 4/√π * (m/2kT)^(3/2) * v²*e^[-mv²/2kT]

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14
Q

Maxwell-Boltzmann Energy Distribution

A

f(E) = 2/√π * (1/kT)^(3/2) * E^(1/2)*e^[-E/kT]

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15
Q

Calorie and Joule

A

1cal = 4.184J

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16
Q

Heat Capacity

A

C = Q/ΔT

17
Q

Heat Capacity at Constant Volume and Constant Pressure

A 
Cv = Qv/ΔT
Cp = Qp/ΔT
18
Q

Specific Heat Capacity and Molar Specific Heat

A 
c = C/m
c' = C/n
19
Q

Heat Capacity and Internal Energy

A

Cv = dEint/dT

20
Q

Heat Capacity for an Ideal Gas

A

Cp - Cv = nR

21
Q

Heat Capacity at Constant Volume

Monatomic and Diatomic Ideal Gases

A

monatomic: Cv = 3/2 nR
diatomic: Cv = 5/2 nR

22
Q

Latent Heat of Fusion

A

Energy required to melt a substance
Qf = mLf

Lf of water = 333.5 kJ/kg

23
Q

Latent Heat of Vaporisation

A

Energy required to vaporise a liquid
Qv = mLv

Lv of water = 2257 kJ/kg

24
Q

First Law of Thermodynamics

A

The change in the internal energy of a system equals the energy transferred into the system via heat plus energy transferred into the system via work.
ΔEint = Qin + Won

25
Q

Internal Energy

A

The internal energy of a system is a property of the state of a system, as are the pressure, volume, and temperature. Heat and work are not properties of state.
Eint of an ideal gas depends only on the temperature T.
dEint = CvdT

26
Q

Internal Energy of a Monatomic Ideal Gas

A

Eint = 3/2 nRT

27
Q

Quasi-Static Process

A

A quasi-static process is one that occurs slowly so that the system moves through series of equilibrium states.

28
Q

Isometric/Isochoric, Isobaric, Isothermal, Adiabatic

A 
Isometric/Isochoric = constant volume
Isobaric = constant pressure
Isothermal = constant temperature
Adiabatic = Q=0
29
Q

Adiabatic Process for an Ideal Gas

A

TV^(γ-1) = constant
PV^γ = constant
Tγ / P^(γ-1) = constant

γ = Cp/Cv

30
Q

Work Done on a Gas

A

Won = - (Vf,Vi) ∫ PdV

31
Q

Work Done on a Gas

Isometric

A 
Vf = Vi
Won = 0
32
Q

Work Done on a Gas

Isobaric

A

Won = - (Vf,Vi) ∫ PdV = -P* (Vf,Vi) ∫ dV = -PΔV

33
Q

Work Done on a Gas

Isothermal

A

Won = - (Vf,Vi) ∫ PdV = -nRT(Vf,Vi) ∫ 1/VdV = nRTln(Vi/Vf)

34
Q

Work Done on a Gas

Adiabatic

A

Won = Cv*ΔT

35
Q

Failure of the Equipartition Partition Theorem

A

The equipartition theorem fails if the thermal energy (~kT) that can be transferred in collisions is smaller than the energy gap ΔE between quantised energy levels. E.g. monatomic gas molecules cannot rotate because the first non-zero energy permitted is much greater than kT.

36
Q

Dulong-Petit Law

A

The molar specific heat of most solids is 3R.

This is predicted by the equipartition theorem assuming that a solid atom has 6 degrees of freedom.

Physics Revision Year 1 (7 decks)

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