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Ch. 6

what is a system the matter that is being observed. The total amount of reactants and products in a chem. rxn. The solute and solvent used to create a solution
isolated system cannot exchange energy (heat and work) or matter with the surroundings; for example, an insulated bomb calorimeter
closed system the system can exchange energy (heat and work) but not matter with the surroundings. for example, a steam radiator
open system the system can exchange both energy (heat and work and matter with the surroundings. for example, boiling water
process when a system experiences a change in one or more of its properties (concentration of reactant or product, temp, or pressure) associated with changes of state system
isothermal process when the system's temp is constant. constant temp implies that the total internal energy of the system is constant throughout process
adiabatic process no heat is exchanged between the system and the environment. thus heat content of the system is constant throughout the process
isobaric process pressure of system is constant.
what are the state functions temperature, pressure, volume, density, internal energy (E or U), enthalpy(H), entropy(S), and Gibb's free energy (G). when state of system changes from equilibrium one of these must change
standard conditions 25 degrees C, (298K) and 1atm
Heat (Q) the transfer of energy from one substance to another as a result of their differences in temp. heat is a process function, not a state function
first law of thermodynamics change in the total internal energy (delta U) of system is equal to the amount of heat(thermal E) transferred(Q) to system, minus amount of W done by system. DeltaU=Q-W
endothermic process in which system absorbs heat (+DQ)(+DH).
exothermic process in which the system releases heat (-DQ)(-DH)
equation for how much heat is released or absorbed in a process q=mcDT m=mass, c=specific heat, DT=change in temp.
enthalpy (H) way to express heat changes at constant pressure. the change in enthalpy is equal to the heat transferred into or out of the system at constant pressure. DHrxn = Hproducts - Hreactants
standard enthalpy of formation the enthalpy change that would occur if one mole of a compound in its standard state were formed directly from its elements in their respective standard states. DH^0f of an elements in its standard state is 0
standard heat of a reaction DH^orxn is the hypothetical enthalpy change that would occur if the reaction were carried out under standard conditions. this means that all reactants and products must be in there standard states.
Hess's law enthalpy changes of reactions are additive. When thermochemical equations are added to give net equation for a rxn, the corresponding heats of rxn are also added to give net heat of rxn
bond dissociation energy the average energy that is required to break a particular type of bond between atoms in the gas phase (endothermic process) given as kJ/mol of bonds broken. Bond formation has same magnitude of energy but is positive.
second law of thermodynamics energy spontaneously disperses from being localized to becoming spread out if it is not hindered from doing so.
entropy the measure of the spontaneous dispersal of energy at a specific temperature: how much energy is spread out, or how widely spread it becomes in the process.
Gibbs free energy a measure of the change in enthalpy and entropy as a system undergoes a process. the change in free energy is the maximum amount of energy released by a process, occurring at constant temp and pressure. DG=DH-TDS
Delta G and rxns DG>0 rxn is spontaneous. DG<0 rxn is non spontaneous. DG=0 rxn is in a state of equilibrium thus DH=TDS
effects of H and S on G (-H +S spontaneous at all temps) (+H -S non spontaneous at all temps) (+H +S spontaneous only at high temps) (-H -S spontaneous only at low temps)
boiling point temperature at which the vapor pressure equals the ambient pressure
Free energy and Keq DG^orxn = -RTlnKeq. the greater the value of Keq is, the more possitive the value of its natural log, the more negative the standard free energy change. The more negative the standard free energy change, the more spontaneous the reaction.
DGrxn = RTln(Q/Keq) if ration of Q/Keq is less than one (Q<Keq), then ln will be negative, so the rxn will spontaneously proceed forward to equilibrium. Q/Keq greater than one (Q>keq) ln positive, G+, move reverse until equilibrium reached. Q=Keq then at equilibrium
Laws of thermodynamics in equations DEsyt + DEsurr = DEuniv, DSsys + DSsurr = DSuniv, Suniv = 0 at 0K
entropy a measure of the disorder of a system
specific heat the amount of heat needed to raise the temperature of one unit of mass of a substance by one degree celcius
heat capacity the amount of heat needed to raise the temperature of a substance by one degree centigrade
Created by: adam87
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