P Chem
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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thermodynamics | study of transformation of energy
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system | the quantity of matter when we can draw a boundary
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surroundings | region outside system we make measurements
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open system | matter and energy CAN be transferred through boundry between system and surroundings
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closed system | matter CANNOT be transferred through boundry. Energy CAN be transferred.
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isolated system | closed system that has no mechanical/thermal contact with surroundings CANNOT transfer matter or energy
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work | done to achieve motion against an opposing force:Raise weight. when a force acts upon an object to cause displacement of an object. eg. Pushing shoprite cart.
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energy | capacity to do work
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heat | energy transferred due to temp. differences ONLY
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diathermic | boundries that DO permit transfer of energy as heat
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adiabatic | boundries that do NOT permit transfer of energy as heat
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exothermic | releases energy as heat into suroundings. combustion increase TEMP
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endothermic | energy is absorbed by sustem from surroundings as heat
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thermal motion | disorderly molecular motion in surroundings.
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internal energy | total energy of system state function deyltaU
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state function | value depends only on current state of system independent of path
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first law of thermodynamics | internal energy of an isolated system is constant
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expansion work | work arising from change in volume
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nonexpansion work/ additional work | work arising from no change in volume
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free expansion | expansion against zero opposing force
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indicator diagram | graph used to show expansion of work
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reversible change | change that can be reversed by an infinitesimal ,small modification of a variable.
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calorimetry | study of heat transfer during physical and chemical process.
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calorimeter | device used to measure energy energy transferred as heat
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adiabatic bomb calorimeter | measures internal energy when q=0
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calorimeter constant | c
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heat capacity | slope tangent to curve at any temp
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molar heat capacity | Cvm=Cv/n
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specific heat capacity | Cv/mass
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enthalpy | u+pV
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isobaric calorimieter | constant pressure
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adiabatic flame calorimeter | constant volume
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differential scanning calorimeter | measure H
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thermochemistry | study of energy transferred as heat in chem rxn
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std enthalpy | change in enthalpy when the inital and fianl substances in std state
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std state | 1 bar
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std enthalpy of transition | change in physical state
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hfus | s to l
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hvap | l to g
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lattice enthalpy | change in std molar enthalpy
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born haber cycle | solves for lattice enthlpy
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thermochemical equation | combo of chem eq and corresponding change in std enthalpy
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std reaction enthalpy | sum of H prod - Sum of Hreac
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std enthalpy combustion | complete oxidation of organic compound to co2 gas and liquid h2o is contains CHON
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hess law | enthalpy of an overall rxn is the sum of std enthalpies of individual rxns into which a rxn maybe divided.
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std enthalpy of form | std rxn enthalpy for formation of compound from its elements in ref states.
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reference state | most stable state 1 bar
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stochimetric numbers | vj Hprod-Hreac
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kirchoff Law | equates emission and absorption in heated objects
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path functions | depend on path between 2 states
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exact differential | small quanitity when integrated gives a result that is independent of path between initial and final state.
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inexact differential | small quantity when integrated gives a result that depends on path between initial and final states.
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internal pressure | internal energy of system changes when it expands or contracts at constant temp
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expansion coeff | fractional change in volume when temp increases
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isothermal compressibility | fractional change in volume when pressure increases
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isenthalpic | constant enthalpy
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isothermal joule thomson coeff | slope of graph p vs t
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inversion temp | critical temp when non ideal gas is expanding at constant enthalpy temp is decreasing.
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eida
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