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33 Cards in this Set
- Front
- Back
work
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done when an object is moved against an opposing force
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energy
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the capacity to do work
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heat
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energy transfer as a result of a temperature difference between the system and its surroundings
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diathermic
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boundary if a change of state is observed when two objects at different temperatures are brought into contact
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adiabatic
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boundary in which there is no heat or matter exchange
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exothermic process
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releases energy as heat into its surroundings
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endothermic process
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energy is acquired from its surroundings as heat
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thermal motion
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disorderly movement of molecules as a result of a transfer of energy
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expansion work
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motion arising from a change in volume
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non-expansion work
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additional motion
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additional work
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non-expansion motion
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free expansion
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movement against zero opposing force
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indicator diagram
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a p,V-graph used to illustrate expansion work
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reversible change
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alteration that can be turned around by an infinitesimal modification of a variable
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calorimetry
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the study of heat transfer during physical and chemical processes
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calorimeter
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a device for measuring energy transferred as heat
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adiabatic bomb calorimeter
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most common device for measuring energy transferred as heat
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calorimeter constant
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measured electrically by passing a steady current from a source of known potential difference through a heater for a known period of time; used for calibration purposes; can also be determined by burning a known mass of substance that has a known heat output
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heat capacity
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the slope to the tangent of the curve of internal energy vs. temperature
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heat capacity at constant volume
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(dU / dT)V
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molar heat capacity at constant volume
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intensive property; transfer of energy due to temperature difference per mole of substance
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specific heat capacity
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ability to transfer energy due to temperature difference divided by mass
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internal energy
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total capacity of a system to do work
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state function
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in which the value depends only on the current condition of the system and is independent of how that condition has been prepared
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First Law of thermodynamics
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The internal energy of an isolated system is constant.
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enthalpy
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H = U + pV; a measure of the total energy of a thermodynamic system
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isobaric calorimeter
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a measuring device for studying processes at constant pressure
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adiabatic flame calorimeter
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used to measure the change in temperature when a given amount of substance burns in a supply of oxygen
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differential scanning calorimeter
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thermoanalytical technique in which the difference in the amount of heat required to increase the temperature of a sample and reference is measured as a function of temperature; most sophisticated way to measure enthalpy changes
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heat capacity at constant pressure
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the slope of the tangent to a plot of enthalpy against temperature at a steady force per unit area
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molar heat capacity at constant pressure
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transfer of energy due to temperature difference per mole of material at a steady force per unit area
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adiabat
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the curves of pressure versus volume for changes in which there is no heat or matter exchange
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thermochemistry
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the study of the energy transferred as heat during the course of a reaction
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