Topic 3 - Thermal Physics

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10 Terms

1

Temperature (unit: ℃ or K)

A measure of the average kinetic energy (per particle) of a system.

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2

Heat (unit: J)

Energy transfer due to a temperature difference.

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3

Internal Energy (unit: J)

The total kinetic and potential energy of the system. Note: For ideal gases, this energy is all kinetic

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4

Heat capacity (unit: J K-1)

The amount of energy required to raise the temperature of a system by 1K

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5

Specific Heat capacity (unit: J kg-1 K-1)

The amount of energy per unit mass required to raise the temperature of a given substance by 1K

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6

Assumptions made for an ideal gas

  1. The particles are in constant, random motion, only interacting through elastic collisions with each other and container walls.

  2. A large number of identical particles with volumes negligible compared to the container volume.

  3. Low density, which typically is the case for low pressure and high temperature

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7

Specific latent heat of vaporization (unit: J kg-1)

The energy needed to convert one unit mass of liquid of a given substance to gas.

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8

Specific latent heat of fusion (unit: J kg-1)

The energy needed to convert one unit mass of solid of a given substance to liquid.

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9

Why temperature remains constant during state change

  • Intermolecular bonds are formed during freezing

  • Intermolecular PE decreases and difference transferred as heat

  • Average KE of molecules does not decrease/change

  • Temperature is related to average KE of molecules hence unchanged

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10

Outline the difference between the molecular structure of a solid and a liquid

  • in solid state, nearest neighbour molecules cannot exchange places/have fixed positions/are closer to each other/have regular pattern/have stronger forces of attraction

  • in liquid, bonds between molecules can be broken and re-form

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