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| the study of the relationship between chemistry and energy |
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| the result of a force acting through a distance |
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| the flow of energy caused by a temperature difference |
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| the energy associated with motion of an object |
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| a type of kinetic energy associated with the temperature of an object, arising from the motion of individual atoms or molecules in the object |
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| the energy associated with the position or composition of an object |
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| the energy associated with the relative positions of electrons and nuclei in atoms and molecules |
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| law of conservation of energy |
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| a law stating that energy can neither be created nor destroyed, only converted from one form to another |
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| in thermodynamics, the portion of the universe which is singled out for investigation |
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| in thermodynamics, everything in the universe which exists outside the system under investigation |
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| the SI unit for energy; equal to 1 kg x m squared/s squared |
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| a unit of energy defined as the amount of energy required to raise one gram of water 1 degree C; equal to 4.184 J |
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| shorthand notation for the kilocalorie (kcal), or 1000 calories |
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| an energy unit used primarily to express large amounts of energy produced by the flow of electricity; equal to 3.60 x 10^6 J |
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| the general study of energy and its interconversions |
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| first law of thermodynamics |
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| the law stating that the total energy of the universe is constant |
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| the sum of the kinetic and potential energies of all of the particles that compose a system |
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| a function whose value depends only on the state of the system, not on how the system got to that state |
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| the point at which there is no additional net transfer of heat between a system and its surroundings |
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| the quantity of heat required to change a system;s temperature by 1 degree C |
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| specific heat capacity (Cs) |
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| the amount of heat required to raise the temperature of 1 g of a substance by 1 degree C |
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| the amount of heat required to raise the temperature of one mole of a substance by 1 degree C |
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| the work that occurs when a volume change takes place against an external pressure |
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| the experimental procedure used to measure the heat evolved in a chemical reaction |
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| a piece of equipment designed to measure change in Erxn for combustion reactions at constant volume |
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| the sum of the internal energy of a system and the product of its pressure and volume; the energy associated with the breaking and forming bonds in a chemical reaction |
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| a chemical reaction that absorbs heat from its surroundings; change in H > 0 |
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| a chemical reaction that releases heat to its surrounds; change in H < 0 |
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| enthalpy (heat) of reaction (change in Hrxn) |
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| a piece of equipment designed to measure change in Hrxn for reactions at constant pressure |
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| the law stating that if a chemical equation can be expressed as the sum of a series of steps, then change in Hrxn for the overall equation is the sum of the heats of reactions for each step |
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| for a gas the standard state is the pure gas at a pressure of exactly 1 atm; for a liquid or solid the standard state is the pure substance in its most stable form at a pressure of 1 atm and the temperature of interest (often taken to be 25 degrees C); for a substance in solution the standard state is a concentration of exactly 1 M |
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| standard enthalpy change (change in H degrees) |
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| the change in enthalpy for a process when all reactants and products are in their standard states |
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| standard enthalpy of formation (change in H degrees f) |
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| the change in enthalpy when 1 mol of a compound forms from its constituent elements in their standard states |
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