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Physics > Thermal physics & Ideal gases > Flashcards

Thermal physics & Ideal gases Flashcards

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1
Q

Definition

Internal energy

A

Sum of random kinetic and potential energies of the atoms in a system

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2
Q

Definition

First law of thermodynamics

A

Increase internal energy = thermal energy transferred + work done on a body

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3
Q

Formula

Work done equals

A

Pressure * Change in volume

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4
Q

Definiton

Isothermal change

A

Change of a system where the temp remains constant

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5
Q

Definition

Specific heat capacity

A

Energy required by unit mass per unit temperature change

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6
Q

Formula

Specific heat capacity equals

A

E / (Mass * Change in Temp)

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7
Q

Definition

Specific latent heat of fusion

A

Amount of heat energy per unit mass needed to convert solid to liquid without change in temp

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8
Q

Definition

Specific latent heat of vaporization

A

Amount of heat energy per unit mass needed to convert liquid to gas without change in temp

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9
Q

Formula

Specific latent heat equals

A

Energy / Mass

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10
Q

Definition

Heat energy (Thermal energy)

A

Energy transferred from one object to another because of a temp change

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11
Q

Definition

Absolute zero

A

Temperature where a system has minimum internal energy (0K or -273C)

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12
Q

Definition

Boyle’s law

A

The pressured exerted by a fixed mass of gas is inversely proportional to its volume, if temp is constant

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13
Q

Definition

Charles’s law

A

Volume occupied by a gas at constant temp is directly proportional to its thermodynamic temp

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14
Q

Definition

Ideal gas

A

Gas that behaves according to the equation pV = NRT

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15
Q

Formula

2 Ideal gas equations

A

pV = nRT
pV = NkT

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16
Q

Definition

Kinetic theory of gases (Volume)

A

Volume of particle is neglegible compared to volume of gas (as liquid boils to become gas, particles become further apart)

17
Q

Definition

Kinetic theory of gases (Force)

A

Force between particles are negligible, except during collision (if attracted strongly, they would end up in the middle of the container)

18
Q

Definition

Kinetic theory of gases (Time of collision)

A

Time of collision with walls is negligible compared with the time between collisions (molecules considered as hard spheres)

19
Q

Definition

Kinetic theory of gases (number of particles)

A

Large number of particles moving random that collide elastically with walls and with each other (Internal energy of gas is the total kinetic energy of the particles)

20
Q

Formula

Pressure of an ideal gas equals

A

p = 1/3 * (Number of molecules * Mass / Volume) * mean_square speed

21
Q

Formula

Kinetic energy of a molecule equals

A

3/2 * k * Temp

22
Q

Definition

Root mean square speed

A

The square root of the average of the squares of the speeds of all the molecules in a gas

Physics (10 decks)

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