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Definition
| The theoretical lowest temperature possible, which occurs when all random motion of molecules has ceased |
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| The temperature at which a phase change of liquid to gas takes place through boiling. It is the same temperature as the condensation point |
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| Celsius scale of temperature |
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Definition
| In the celsius scale of temperature, the ice-point is taken as taken as the lower fixed point (0 deg C ) and the steam-point is taken as the upper fixed point (100 deg C). The interval between the ice point and steam point is divided into 100 equal divisions. Thus, the unit division on this scale is 1degC. This scale was earlier called the centigrade scale. 1 deg C = 9/5 deg F. |
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| Alternate name for the Celsius scale |
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| Coefficient of volume expansion |
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Definition
| The increase in volume of a substance per unit original volume per degree rise in temperature is called its coefficient of cubical expansion. The SI unit of coefficient of cubical expansion is K-1. |
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| Coefficient of linear expansion |
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Definition
| The increase in length per unit original length per degree rise in temperature is called the coefficient of linear expansion. The SI unit of the coefficient of linear expansion is K-1. |
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| The transfer of heat from a region of higher temperature to a region of lower temperature by increased kinetic energy moving from molecule to molecule |
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Heat of Fusion
The energy required to change a gram of a substance from the solid to the liquid state without changing its temperature is commonly called it's "heat of fusion". This energy breaks down the solid bonds, but leaves a significant amount of energy associated with the intermolecular forces of the liquid state. |
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Heat of Vapourization
The energy required to change a gram of a liquid into the gaseous state at the boiling point is called the "heat of vaporization". This energy breaks down the intermolecular attractive forces, and also must provide the energy necessary to expand the gas (the PDV work). For an ideal gas , there is no longer any potential energy associated with intermolecular forces. So the internal energy is entirely in the molecular kinetic energy. The final energy is depicted here as being in translational kinetic energy, which is not strictly true. There is also some vibrational and rotational energy. |
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| The transfer of heat from a region of higher temperature to a region of lower temperature by greater emission of radiant energy from the region of higher temperature |
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| Transfer of heat from a region of higher temperature to a region of lower temperature by the displacement of high-energy molecules-for example, the displacement of warmer, less dense air (higher kinetic energy) by cooler, denser air (lower kinetic energy) |
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| Heat is a form of energy, which makes a body hot or cold. Heat is measured by the temperature-effect it produces in any material body. The SI unit of heat is Joule( J). |
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| - energy in motion. Kinetic energy is the greatest in gases and least in solids. |
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| - stored energy. Potential energy is the greatest in solids and least in gases. |
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| - the quantity of heat (energy) needed to raise the temperature of unit of mass of a substance by a unit of temperature change. |
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| The First Law of Thermodynamics |
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Definition
(a restatement of the Law of Conservation of Energy) states:
The quantity of heat energy transferred to a system is equal to the work done by the system plus the change in the internal energy of the system
You can't Win |
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Term
| Second Law of Thermodynamics. |
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Definition
Natural Processes go in a direction that increases the ENTROPY of the system
The natural flow of heat is from a hot object to a cold object.
Another way of saying the 2nd law is that energy, when converted from one form to another, can only be lost and not gained.
You Can't Loose |
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| The Third Law of Thermodynamics |
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Definition
states:
Therman Energy is conserved within a closed system.
Absolute zero can never be reached.
You can't get out of the Game |
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Definition
everything moves toeards becoming More disorganized(to
chaos) |
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