vocabulary terms
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| calorie | amount of heat required to raise the temperature of one gram of pure water by one degree Celsius
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| chemical potential energy | energy stored in a substance because of its composition; most is released or absorbed as heat during chemical reactions or processes.
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| energy | capacity to do work or produce heat; exists as potential energy, whish is stored in an object due to its composition or position, and kinetic energy, which is the energy of motion.
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| heat | form of energy that flows from a warmer object to a cooler object.
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| joule | SI unit of heat and energy
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| law of conservation of energy | states that in any chemical reaction or physical process that energy may change from one form to another, but it is neither created nor destroyed
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| specific heat | amount of heat required to raise the temperature of one gram of a given substance by one degree Celsius
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| calorimeter | an insulated device that is used to measure the amount of heat released or absorbed during a physical or chemical process.
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| enthalpy | heat content of s system at constant pressure.
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| enthalpy (heat) of reaction | change in enthalpy for a reaction- the difference between the enthalpy of the substances that exist at the end of the reaction and the enthalpy of the substances present at the start.
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| surroundings | in thermochemistry, includes everything in the universe except the system.
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| system | in thermochemistry, the specific part of the universe containing the reaction or process being studied.
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| thermochemistry | the study of heat changes that accompany chemical reactions and phase changes
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| universe | in thermochemistry, is the system plus the surroundings
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| enthalpy (heat) of combustion | the enthalpy change for the complete burning of one mole of a given substance
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| molar enthalpy (heat) of fusion | amount of heat required to melt one mole of a solid substance
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| molar enthalpy (heat) of vaporization | amount of heat required to vaporize one mole of a liquid
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| thermochemical equation | balanced chemical equation that includes the physical states of all of the reactants and the energy change, usually expressed ass the change in enthalpy.
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| Hess's law | states that if two or more thermochemical equations can be added to produce a final equation for a reaction, then the sum of the enthalpy changes for the individual reactions is the enthalpy change for the final reaction.
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| standard enthalpy (heat) of formation | change in enthalpy the accompanies the formation of one mole of a compound in its standard state from its constituent elements in their standard states
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| entropy | measure of the number of possible ways that the energy of a system can be distributed; related to the freedom of the system's particles to move and the number of ways they can be arranged.
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| free energy | energy available to do work; difference between the change in enthalpy and the product of the entropy change and the kelvin temperature
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| second law of thermodynamics | spontaneous processes always proceed in such a way that the entropy of the universe increases
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| spontaneous process | a physical or chemical change that occurs without outside intervention and may require energy to be supplied to begin the process.
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