HONORS CHEMISTRY Unit G: ENERGY, KINETICS, and...
Transcript of HONORS CHEMISTRY Unit G: ENERGY, KINETICS, and...
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HONORS CHEMISTRYUnit G: ENERGY, KINETICS, and EQUILIBRIUM
CHAPTER SIXTEEN: REACTION ENERGY
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THERMOCHEMISTRYuCHEMICAL REACTIONS are
accompanied by an ENERGY CHANGEuChemical bonds BREAK & REFORM – absorbing
and releasing energy in a reactionuPHASE CHANGES also absorb or release energyuTHERMOCHEMISTRY is the study of energy
transfer as HEAT in chemical reactions or phase changes
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HEAT & TEMPERATUREuTEMPERATURE (T) is a measure of
the average KE of particles in a sample of matter (ºC or K)
uHEAT (q) is the energy transferred between matter at different temps (Joule (J) or (kJ))
uTHESE TWO THINGS ARE DIFFERENT!
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HEAT & TEMPERATURE
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HEAT & TEMPERATURE
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SPECIFIC HEATuSPECIFIC HEAT is the amount of energy
required to raise the temperature of 1 g of a substance by 1 K or 1ºC
uUnit: (J/g・ºC)uSPECIFIC HEAT à (c)uSpecific Heat of Water = 4.18 J/g・ºCuSPECIFIC HEAT (c) & HEAT (q) ARE TWO
DIFFERENT THINGS!
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SPECIFIC HEATuSPECIFIC HEAT is dependent upon the
identity of the substanceuSPECIFIC HEAT quantitatively describes
heat transfer ability of a substance
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CALORIMETERuCALORIMETER is the instrument used to measure
HEAT involved or transferred in a reactionuCan be used to measure ENTHALPY CHANGEuENTHALPY CHANGE is the amount of energy (heat)
gained or lost during a reaction or phase change
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CALORIMETER
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ENTHALPY of REACTIONuENTHALPY OF REACTION is the quantity of energy
transferred as HEAT during a chemical reactionuSometimes called “Heat of Reaction”uEnthalpy of reaction = △Hrxn
uThe difference between the energy stored in the bonds of the reactants and products
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ENTHALPY of REACTIONuEXOTHERMIC REACTIONS release energy as a
“PRODUCT” (HEAT OUT – HOT)uENDOTHERMIC REACTIONS absorb energy as a
“REACTANT” (HEAT IN – COLD)uTHERMOCHEMICAL EQUATIONS include the △Hrxn
in the equation
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ENTHALPY of REACTION
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THERMOCHEMICAL EQUATIONS
uThe equations represent molar amounts and the △Hrxn is proportional to the molar amounts
uPhysical states must be includeduThe sign reverses if the equation reversesu Temperature is not
important
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ENTHALPY OF FORMATIONuENTHALPY OF FORMATION is the enthalpy change
that occurs when one mole of a compound forms from its elements @ standard conditions (product)
u△H0f = ENTHALPY OF FORMATION
u△H0f = 0 (for elements in standard state)
u△H0f is NEGATIVE for STABLE COMPOUNDS
u△H0f is POSITIVE FOR UNSTABLE COMPOUNDS
uUsually obtained from a reference tableuUseful for HESS’S LAW CALCULATIONS
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HESS’S LAWuHESS’S LAW uses thermochemical equations for
reactionsuThe parts of a reaction SUM to the wholeuHESS’S LAW is that the overall enthalpy change in
a reaction is equal to the sum of the individual steps of the process
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HESS’S LAWuThe component equations are always provideduIf the reaction needs to be reversed, then reverse
the △H0f sign (+ to -) or (- to +)
uSometimes multiply the equation to give desired stoichiometric values, then also multiply the △H0
fvalue
uIT’S A LITTLE TRICKY, BUT HANG IN THERE!
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SEE THE SAMPLE PROBLEMS IN THE
TEXTBOOK FOR MORE!
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ENTHALPY?~ENERGY!
...△H…EXOTHERMIC (-△H)
…ENDOTHERMIC (+△H) …HEAT & q
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REACTIONS: DRIVING FORCES
uReactions can be SPONTANEOUS (favorable) or NON-SPONTANEOUS (unfavorable)
uTwo factors determine SPONTANIETY:uENTHALPY (energy) (H)uENTROPY (disorder) (S)
uENTROPY is the degree of randomness of particles
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REACTIONS: DRIVING FORCES
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REACTIONS: DRIVING FORCES
uMost reactions are exothermic (favorable △H )uEndothermic reactions rare (unfavorable △H)uHOW ARE ENDOTHERMIC REACTIONS POSSIBLE?uENTROPY (disorder) make endothermic reactions
possibleu△S is the change in ENTROPY (disorder)
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ENTROPY (△S)
u+△S = increased disorder (favorable)u-△S = decreased disorder (unfavorable)uThe production of “more moles” of products or
products in a higher energy physical state have +△S (greater entropy)
u(s) < (l) < (aq) < (g)u 2 HN4NO3 (s) à 2 N2 (g) + 4 H2O (l) + O2 (g)
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ENTROPY (△S)
uNaturally occurring reactions tend to favor greater disorder ( HIGHER ENTROPY)
uMelting, decomposition, solutionsu△S units: (kJ/mol・K)uHOWEVER… it is possible to for a system to
become MORE ORDERED (LOWER ENTROPY)!
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ENTHALPY & ENTROPY uNatural process are driven in 2 directions:uLOWER ENTHALPY (energy) -△HuHIGHER ENTROPY (disorder) +△SuThe two forces can work together or oppose each
otheruGIBBS FREE ENERGY (△G) is a function of
ENTHALPY and ENTROPY and is TEMPERATURE dependent
uPREDICTS SPONTANEITY OF REACTION (△G)
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GIBBS, ENTHALPY & ENTROPY: △G, △H, △S
uREACTIONS BOTH EXOTHERMIC (-△H) AND INCREASE DISORDER (+△S) à SPONTANEOUS
uReactions can be endothermic and still spontaneous
uReactions can be more ordered and still be spontaneous
uREACTIONS BOTH ENDOTHERMIC (+△H) AND DECREASE DISORDER (-△S) à NOT SPONTANEOUS
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GIBBS FREE ENERGY
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GIBBS FREE ENERGY
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GIBBS FREE ENERGY
u-△G = SPONTANEOUS (will happen)
u+△G = NOT SPONTANEOUS (won’t happen)