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| the study of energy and its transformation |
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| the relationship between chemical reactions and energy changes |
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| the energy that an object possesses by virtue of its motion |
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| the energy that an object possesses as a result of its composition or its position with respect to another object |
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| the SI unit of energy 1 kg*m^2/s^2; 4.184 J = 1 calorie |
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| a unit of energy, it is the amount of energy needed to raise the temperature of 1 g of water 1*C |
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| in thermodynamics, the portion of the universe that we single out for study; we must be careful to state exactly what the system contains and what transfers of energy it may have with its surroundings |
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| in thermodynamics, everything that lies outside the system that we study |
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| the movement of an object against some force |
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| the flow of energy from a body at higher temperature to one at lower temperature when they are placed in thermal contact |
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| the capacity to do work or to transfer heat |
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| the total energy possessed by a system; when a system undergoes a change, the change in internal energy is defined as the heat added to the system |
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| first law of thermodynamics |
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Definition
| a statement that energy is conserved in any process; one way to express the law is that the change in internal energy of a system is any process is equal to the heat added to the system plus the work done on the system |
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| a process in which a system absorbs heat from its surroundings |
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| a process in which a system releases heat to its surroundings |
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| a property of a system that is determined by its state or condition and not by how it got to that state; its value is fixed when temperature, pressure, composition, and physical form are specified |
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| work performed by expansion of a gas against a resisting pressure |
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| a quantity defined by the relationship H = E + PV; the enthalpy change for a reaction that occurs at constant pressure is the heat evolved or absorbed in the reation |
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| the enthalpy change associated with a chemical reaction |
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| the experimental measurement of heat produced in chemical and physical processes |
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| an apparatus that measures the heat released or absorbed in a chemical or physical process |
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| the quantity of heat required to raise the temperature of a sample of matter by 1*C |
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| the heat required to raise the temperature of one mole of substances by 1*C |
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| the heat capacity of 1 g of a substance; the heat required to raise the temperature of 1 g of substance by 1*C |
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| a device for measuring the heat evolved in the combustion of a substance under constant volume conditions |
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| the heat evolved in a given process can be expressed as the sum of the heats of several processes that when added, yield the process of interest |
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| the enthalpy change that accompanies the formation of a substance from the most stable forms of its component elements |
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| the change in enthalpy in a process when all reactants and products are in their stable forms at 1 atm pressure and a specified temperature, commonly 25*C |
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| standard enthalpy of formation |
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Definition
| the change in enthalpy that accompanies the formation of one mole of a substance from its elements, with all substances in their standard states |
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| the energy released when 1 g of a substance is combusted |
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| coal, oil, and natural gas, which are presently our major sources of energy |
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| a naturally occurring mixture of gaseous hydrocarbon compounds composed of hydrogen and carbon |
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| a naturally occurring combustible liquid composed of hundreds of hydrocarbons and other organic compounds |
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| a naturally occurring solid |
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| energy such as solar energy, wind energy, and hydroelectric energy derived from essentially inexhaustible sources |
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