When two objects reach the same temperature (after flow from hot to cold) by transferal of thermal energy (heat)
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Relation between celsius and kelvin.
T (K) = t (in celsius) +273, 0 degrees celsius = 273 degrees kelvin
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Define internal energy.
The total potential energy and random kinetic energy of the molecules of the substance
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Define mole.
SI-unit for amount of substance. One mole of any substance is equal to the amount of that substance that contains the same number of atoms as 0.012 kg of carbon-12.
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Define molar mass.
the mass of one mole of a substance in g.
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Define specific heat capacity
Amount of heat required to raise the temperature of 1 kg of a material by 1 degree celsius. Unit: J/kg/C c=Q/(m*deltaT) *Does not depend on size of object, only what it is made of
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Avogadro's constant
Number of atoms in 0.012 kg of carbon-12. it is 6.02*10^23
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Temperature
measure of average kinetic energy of the molecules in a substance
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Define thermal capacity
C of an object as the energy required to raise its temperature by 1 K:
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The solid state.
Fixed shape and volume. Molecules held together by a force, they vibrate but don't move around.
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The liquid state.
No fixed shape, however fixed volume. Force between molecules is not very strong and the molecules are able to move around.
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The gas state.
No fixed shape nor volume. No force (ideally) between molecules so they move around freely.
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Explain internal energy.
When we do work on an objects it enables the molecules to move faster (increasing KE) and move apart (increasing PE) which leads to an increase in internal energy. The energy is "stored" in the object and not lost to surroundings.
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Explain the differences with particles when something is hot or cold.
Cold: molecules vibrate a bit Hot: molecules vibrate faster and are slightly further apart
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Define thermal capacity (värmekapacitet).
Amount of heat needed to raise body's temperature by 1 degree celsius. Unit: J/C c=Q/deltaT *Depends on size ob object and what it is made of
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Change of state: solid --> liquid
Melting.
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Change of state: liquid --> solid
Freezing.
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Change of state: liquid to gas
Vaporisation.
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Change of state: gas --> liquid
Condensation.
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Explain boiling and where it occurs.
Takes place throughout the liquid and always at the same temperature.
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Explain evaporation and where it occurs.
Takes place only at the surface and can happen at all temperatures.
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Why does a liquid get colder during evaporation?
The fastest moving particles (the ones with the highest KE) leave the surface and the remaining average KE is then lower, resulting in a drop in temperature.
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Define specific latent heat.
Amount of heat required to change the state of 1 kg of the material WITHOUT change of temperature. Unit: J/kg L=Q/m
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Define pressure.
Particles exerting continuous force on walls of container. pressure = force/area
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What is absolute zero?
When average KE = zero --> molecules at complete stand-still --> occurs at 0 degrees K or -273 degrees celsius. Gas pressure = zero
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Other cards in this set
Card 2
Front
Define thermal equilibrium.
Back
When two objects reach the same temperature (after flow from hot to cold) by transferal of thermal energy (heat)
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