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33 Cards in this Set
- Front
- Back
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thermodynamics
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study of energy
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energy
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the ability to do work or produce heat
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potential energy
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energy due to position or composition
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kinetic energy
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energy due to the motion of the object and depends on mass
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Law of Conservation of Energy
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energy can be converted to different forms but is always the same amount (can't be created nor destroyed)
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work
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force acting over a distance
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temperature
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measure of the random motion of the components of a substance
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heat
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flow of energy due to a temperature difference
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endothermic
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process that ABSORBS energy from the surroundings into the system
^H is POSITIVE more product potential energy than reactant potential energy |
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exothermic
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process that allows energy to flow OUT of the system
^H is NEGATIVE more reactant potential energy than product potential energy |
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system
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part of the universe on which we want to focus attention (products and reactants)
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surroundings
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everything else in the universe (generally in the room)
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calorie (cal)
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the amount of energy required to raise the temperature of one gram of water by 1 degree C (STP)
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joule (J)
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measures energy and is the unit for the SI System (based upon the energy to move a 1Kg mass of a distance of 1m with a rate of acceleration of 1m/s^2)
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1 cal = ...
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4.184 J
ALSO KNOWN AS THE SPECIFIC HEAT OF WATER |
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formula to calculate energy requirements
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q = (m)(c)(^T)
q = energy required to achieve temperature change (joules) m = mass (grams) c = specific heat capacity of substance (joules per gram degrees Celsius) ^T = change in temperature - T2 - T1 (degrees Celcius) |
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Specific Heat Capacity (c)
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the amount of energy required to change the temperature of one gram of a substance by 1 degree Celsius)
C IS HEAT AND Q IS ENERGY |
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enthalpy (H)
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heat for the reaction
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calorimeter
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device used to determine the heat associated with a chemical reaction
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entropy (S)
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measure of disorder or randomness
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intramolecular forces
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forces that exist within the molecules
example: covalent bonds |
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intermolecular forces
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forces that exist between molecules
example: ion-ion, dipole-dipole, london-dispersion, etc. |
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ion-ion interactions
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the opposite charges of ions attract each other in a crystal structure
metal and a non-metal metal and a polyatomic |
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dipole-dipole attractions
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the attractive force resulting when polar molecules line up such that the positive and negative ends are close to each other
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hydrogen bonding
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type of dipole-dipole attraction between H and F, O, or N
F, O, and N are highly electronegative atoms |
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London-dispersion forces
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a force that exists among noble gas atoms and non polar molecules that involve an accidental dipole that induces a momentary dipole in a neighbor
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heating/cooling curve
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a plot of temperature vs time where energy is added at a constant rate
(solid, solid and liquid, liquid, liquid and gas, gas) |
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Molar Heat of Fusion (^Hf)
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q = (^Hf)(n) ALWAYS IN kJ/mol |
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Molar Heat of Vaporization
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q = (^Hv)(n) ALWAYS IN Kj/mol |
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phase diagram
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represents the areas of stability of the various phases in a chemical system at equilibrium, usually with a respect to pressure and temperature
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triple point (on a phase diagram)
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all states of matter at the same time (not achieved at STP)
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sublimation
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solid to a gas (not achieved at STP)
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critical point (on a phase diagram)
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liquids and gasses morph
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