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32 Cards in this Set
- Front
- Back
defined as the capacity to do work |
energy |
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directed energy change resulting from a process |
work |
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transfer of thermal energy between two bodies |
heat |
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study of heat change in chemical reactions |
thermochemistry |
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specific part of the universe that is of interest to us |
system |
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the rest of the universe outside the system |
surroundings |
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can exchange mass and energy |
open system |
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allows transfer of energy but not mass |
closed system |
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does not allow transfer of mass and energy |
isolated system |
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any process that gives off heat or energy/released |
exothermic process |
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heat has to be supplied to the system by the surrounding/gain |
endothermic process |
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closed container designed specifically to measure heat changes |
calorimeter |
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the measurements if heat changes |
calorimetry |
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amount of heat required to raise the temp. of one gram of substance by one degree celcius |
specific heat |
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amount of heat required to raise the temperature of a given quantity by one degreee celcius |
heat capacity |
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specific heat of water |
4.184 J/g°C |
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steel container filled with oxygen at abount 30 atm |
constant-volume bomb calorimeter |
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used to determine the heat changes for non combustion reactions |
constantl-pressure calorimeter |
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there is net increase in the number of moles |
expansion |
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if more gas molecules are consumed than are produced |
compression |
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shows the enthalpy change as well as the mass relationships |
thermochemical equations |
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deals with the interconversion of heat and other forms of energy |
thermodynamics |
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reaction that does occur under the given set of conditions |
spontaneous reaction |
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is on that, once started, continuous on its own without input of energy |
spontaneous process |
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best indicator of spontaneity in a reaction is the change of? |
entropy |
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what is boltzmann constant? |
1.38×10^-23 J/K |
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each arrangement of energy of each molecule in the whole system at one instant |
microstate |
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defined as the entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process |
second law of thermodynamics |
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what does this implies? ∆G<0 |
The reaction is spontaneous in the forward direction |
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∆G>0 |
The reaction is nonspontaneous. reverse directions |
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∆G=0 |
The reaction is at equilibrium |
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described as a measure of how spread out or dispersed the energy of a system |
entropy |