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42 Cards in this Set
- Front
- Back
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thermodynamics
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the study of energy flow
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thermochemistry
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the study of energy flow in chemical systems
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first law of thermochemistry
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energy can neither be created nor destroyed
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internal energy
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the total of all possible types of energy present in the system. the change in energy (delta E) is the sum of heat plus work
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internal energy formula
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delta E = q+w
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heat
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the amount of thermal energy transferred from one object to another a the result of temperature difference between the two
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work
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is the force that produces the movement of an object times the distance
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formula for work
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w = F x d
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kinetic energy
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the energy of an object in motion
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potential energy
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the amount of energy an object has due to its position
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state function
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function or property whose value depends only on the present state or condition of the system not the path used to arrive at that state
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enthalpy change or delta H
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equal to the change in the internal energy, delta E plus any work done on a system at constant pressure
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system
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the part of the universe being studied
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surroundings
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anything not being studied or everything outside of the system
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open system
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exchange of matter and energy between the system and surroundings
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closed system
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exchange of energy but not matter
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isolated system
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no exchange of energy or matter
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endothermic
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heat flows from the surrounding into the system (qsys = +)
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exothermic
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heat flows to the surrounding from the system (qsys = -)
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calorimetry
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a measurement of the amount of heat transferred
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calorimetry:
heat loss = |
-heat gained
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heat capacity (C)
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amount of heat measured to raise the temperature of 1.00 mole of a substance by 1.00 degree Celsius
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heat capacity formula
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q = msDeltaT
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specific heat
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amount of heat required to raise the temp 1.00g of a substance by 1.00 degrees Celsius
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thermochemical expression
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a balanced chemical equation (including physical states of reactants and products together with a value for delta H
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hess's law of summation
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if a reaction can be written as the sum of two or more steps, then the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes for the individual reactions
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standard conditions
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Conditions of 1.0 bar pressure and 298 k
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standard state
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The physical state of a substance in which it is the most stable under standard conditions
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molar heat of fusion
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amount of heat required to melt one mole of a substance
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molar heat of vaporization
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amount of heat required to vaporize one mole of a substance
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Radiant Energy |
come from the sun and is earths primary energy source |
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Thermal Energy |
Is the energy associated with the random motion of atoms and molecules |
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Chemical energy |
is the energy stored within the bonds of chemical substances |
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Nuclear energy |
is the energy stored within the collection of neutrons and protons in the atom |
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potential energy |
is stored energy or energy of postion that has the potential to do work |
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Kinetic energy |
is the energy of motion |
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Tempertature |
is a measure of the thermal energy |
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Thermochemistry |
is the study of heat change in chemical reactions. |
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Exothermic Process |
is any process that gives off heat- transfers thermal energy from the system to the surrondings. |
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Endothermic process |
is any process in which heat has to be supplied to the system from the surroundings |
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State Functions |
are propertires that are determined by the state of the system, regardless of how that condition was achieved. energy pressure, volume, temperature. |
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First Law of thermodynamics |
energy can be converted from one form to another but cannot be created or destroyed |
