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23 Cards in this Set
- Front
- Back
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Thermodynamics
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study ofheat and work
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energy
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capacity to do work
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kinetic
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energy associated with motion
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potential energy
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energy that results from an object's position
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law of conservation of energy or the First law of thermodynamics
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energy can neither be created or destroyed, the total energy of the universe is constant
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system
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the object, or collection of objects being studied
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surroundings
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everything outside the system that can exchange energy with the system
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thermal equilibrium
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when two objects reach the same temperature. the temperature through the system is the same
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exothermic
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heat is transferred from a system to the surroundings
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endothermic
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heat is transferred from surroundings to the system
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q
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heat transferred
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sys
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system
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joule
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SI unit of thermal energy
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1 calorie =
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4.184 joules
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specific heat cappacity
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quantity of heat required to raise the temp of 1 g of a substance by one kelvin
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q =
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mCAT Joules
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increase +
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heat transferred from surrounds to system (endothermic)
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decrease -
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heat transferred from system to surroundings (exothermic)
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heat of fusion
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heat required to convert a substance from a solid at its melting point to a liquid
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heat of vaporization
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heat required to convert a substance from a liquid to a gas
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sublimation
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property when it absorbs heat from its surroundings changes directly from solid to gas
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internal energy E
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in a chemical system: the sum of the potential and kinetic energies of the atoms, molecules, or ions in the system
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enthalpy (H)
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the heat content of a substance at a constant pressure
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