Topic 3 - Thermal Physics

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10 Terms

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Temperature (unit: ℃ or K)
A measure of the average kinetic energy (per particle) of a system.
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Heat (unit: J)
Energy transfer due to a temperature difference.
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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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Heat capacity (unit: J K-1)
The amount of energy required to raise the temperature of a system by 1K
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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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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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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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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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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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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