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Stack #100963
| Question | Answer |
|---|---|
| thermadynamics | the study of energy and its interconversions |
| the first law of thermodynamics | the energy of the universe is constant |
| state function | a property of a system that depends only on its present state |
| 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 |
| 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 |
| 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 |
| calorimetry | the science of mreasuring heat flows |
| equation for calorimetry | q=mc delta T |
| q is | heat/energy |
| units for q | J |
| c is | scpeicif heat capacity |
| units for c | j per k times g or j per c times h |
| delta t | change in temperature |
| untis for delta t | degrees c or degrees k |
| speciif heat captaicty | the energy required to raise the temperature of one gram of a substaceby on edegree celcius |
| specific heat capacity for water | 4.184 j per c times g |
| molar heat capacity | the energy required to raise the temperature of one mole of as ubstance by one degree celsius |
| symbol for molar heat capacity | cp |
| units for molar heat capacity | kj/k times mol |
| equation for cp | delta H over delta T |
| units for change in T | kelvin |
| extensive properties | propriertes that are depednent on the amount of the substance |
| stoichiometry | to determin the delta h value for a certain amoutn of reactants simply calciulate the value using mole relationsips and stoichiometry |
| phase changes posiitve | melting vaporization sublimation |
| phease changes negative | freezing condenscation deposition |
| 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 |
| characteristics of enthalpy changes | if a reaction is reversed the sign of delta h is also reversed, if its multilied it will be mutiplied |
| 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 |
| symbol for standard enthalpy of formation | delta H degrees F |
| units for standard enthalpies of formation | kj/mol |
| eqation for standard enthalpy of formation | delt H is equal to the sum ofthe products minus the sum of th ereactants |
| delta H degrees f is zero for | all elements |
| pressure is | 1 atm |
| solids liquis and gases are | "pure" |
| soluations are | 1 M |
| bond energy | the nergy required to break a given bond |
| calciulating enthalpy from bond eenergies | delta H is the total of the bonds brown minus the etoal of the bonds formed |
| breaking bonds is | delta H endothermic |
| forming bonds is | - delta H exothermic |
| if a reaction isn't both | thermodynmically and kinestically favored, the reaction won't happen |
Created by:
lilee256