Stack #100963
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| thermadynamics | the study of energy and its interconversions
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| the first law of thermodynamics | the energy of the universe is constant
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| state function | a property of a system that depends only on its present state
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| enthalpy | a property of a system equal to E + PV where E is the internal energy of a ststem, P is the pressure of the system and B is the volume of the system. At constant pressure the change in enthalpy equals the erngy flow as heat
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| exothermic reaction | a reaction where energy flows out of the system, i.e. energy heat is given off to the surroundings, delta H is a product, delta H has a negatiuve value, prodcuts are more stable than reactiants
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| endothermic reaction | a reaction where energy flows into the system, energy/heat is absorbed from the surroundings, delta H is a reactant, delta H has a positiv evalue, reactants are more stable than products
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| calorimetry | the science of mreasuring heat flows
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| equation for calorimetry | q=mc delta T
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| q is | heat/energy
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| units for q | J
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| c is | scpeicif heat capacity
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| units for c | j per k times g or j per c times h
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| delta t | change in temperature
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| untis for delta t | degrees c or degrees k
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| speciif heat captaicty | the energy required to raise the temperature of one gram of a substaceby on edegree celcius
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| specific heat capacity for water | 4.184 j per c times g
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| molar heat capacity | the energy required to raise the temperature of one mole of as ubstance by one degree celsius
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| symbol for molar heat capacity | cp
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| units for molar heat capacity | kj/k times mol
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| equation for cp | delta H over delta T
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| units for change in T | kelvin
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| extensive properties | propriertes that are depednent on the amount of the substance
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| stoichiometry | to determin the delta h value for a certain amoutn of reactants simply calciulate the value using mole relationsips and stoichiometry
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| phase changes posiitve | melting vaporization sublimation
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| phease changes negative | freezing condenscation deposition
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| hess law definition | in going from a partiucular set of reactants to a particular set of products the enthalpy change is the same whether the reaction takes plaece in one step or in a series of steps
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| characteristics of enthalpy changes | if a reaction is reversed the sign of delta h is also reversed, if its multilied it will be mutiplied
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| standard enthalpies of formation | the enthalpy change that accomplanies the formation of one mole of a compound at 25 degrees C from its elements, with all substances in their standard states at te temperature
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| symbol for standard enthalpy of formation | delta H degrees F
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| units for standard enthalpies of formation | kj/mol
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| eqation for standard enthalpy of formation | delt H is equal to the sum ofthe products minus the sum of th ereactants
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| delta H degrees f is zero for | all elements
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| pressure is | 1 atm
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| solids liquis and gases are | "pure"
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| soluations are | 1 M
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| bond energy | the nergy required to break a given bond
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| calciulating enthalpy from bond eenergies | delta H is the total of the bonds brown minus the etoal of the bonds formed
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| breaking bonds is | delta H endothermic
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| forming bonds is | - delta H exothermic
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| if a reaction isn't both | thermodynmically and kinestically favored, the reaction won't happen
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