4.4 how far - entropy
DESCRIPTION
summarised notes on entropyTRANSCRIPT
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Enthalpy changes
The enthalpy changefor a process
is the heat energy exchanged withthe surroundings at constant
pressure.
Enthalpy changes are frequently
measured under standard conditions,
!e! 298Kand100kPa. "f an enthalpychange s measured under standard
condtons, the sym#ol s used n
superscrpt, !H!
Enthalpy change s g$en the sym#ol !H!
%he unts are k&mol'1!
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Enthalpy changes
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Exa"ples of enthalpy changes
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#ond enthalpies
*hen a chemcal reacton takes place, #onds are #roken n
the reactants and #onds are formed n the products! Breakng
#ondss an endother"icprocess! +akng #onds s an
exother"icprocess!
%he "ean $ond enthalpys the a$erage mean-
$ond dissociation enthalpyfor a partcular #ond n
a range of dfferent compounds!
.recsely, t s the a$erage enthalpy change for
#reakng 1 mole of a partcular #ond n a range of
dfferent compounds n the gas phase!
%he enthalpy change for a reacton can #e calculated #y
workng out the enthalpy changes for #onds made and #onds#roken durng the reacton usng mean #ond enthalpes!
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%alculations using $ond enthalpies
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&hat is a #orn'(a$er cycle)
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%onstructing a #orn'(a$er cycle
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#orn'(a$er cycle for *g%l2
*g+s,- %l2+g,
*g+g,- %l2+g,
Ha
+*g, -1/0
*g+g,- 2%l+g,
2
Ha+%l,
2 +-121,
*g-+g,- 2%l+g,- e'
Hi+1st,+*g, -3
Hi+2nd,+*g, -14/0
*g2-+g,- 2%l+g,- 2e'
*g2-+g,- 2%l'
+g,
2
Hea+%l,
2 +'34,
*g%l2+s,
Hl+*g%l2, '249
Hf+*g%l2,
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%an you construct a #orn'(a$er cycle)
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#orn'(a$er cycle 5uestions
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6attice for"ation enthalpies
*hen an onc lattce s formed, the oppostely charged ons
are attracted to each other! %he stronger the attracton, the
hgher the lattce formaton enthalpy!
%wo factors ncrease the attracton and therefore the lattce
formaton enthalpy
hgh charge
small se!
7'2''
6i-7a-K-
increasing lattice for"ation enthalpy
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Polari:ation and lattice enthalpy
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ill in the "issing words; lattice enthalpy
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Enthalpies of solution and hydration
The standard enthalpy of solution
+Hsol, is the enthalpy changewhen one "ole of an ionic
co"pound is dissol
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%alculating enthalpies of solution
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Enthalpy of solution calculations
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actors affecting enthalpy of hydration
%he se of the enthalpy of hydraton depends on
ncreas
ng
s3e
%he charge on the on! %he larger the charge on the on,
the larger the enthalpy of hydraton!
%he se of the on! %he smaller the on, the larger theenthalpy of hydraton!
L
5a
6
'(1
'40)
'322
7'
8l'
Br'
'(0)
'3)4
'33(
=on Hhyd+k>"ol'1, =on Hhyd+k>"ol
'1,
=on Hhyd+k>"ol'1, =on Hhyd+k>"ol
'1,
7e2 7e3'1(0 '4430
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&hat is a spontaneous reaction)
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Entropy
Entropy is a "easure of disorder? and is gi
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Entropy change for reactions
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Predicting entropy changes
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%alculating entropy changes
9tandard entropy changes for any chemcal reacton or
physcal change can #e calculated usng the followng smple
e:presson
;emem#er the followng ponts
entropes of elements are not ero lke Hf$alues, so they
should #e ncluded n calculatons!
the unts of entropy, S, are &6'1mol'1
S Sproducts' S
reactants
% l l i h
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%alculating entropy changes
E t h l l ti
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Entropy change calculations
E t h i th di
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Entropy changes in the surroundings
E t h i th di
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Entropy changes in the surroundings
@i$$ f
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@i$$s free energy
*hether a reacton s spontaneous depends on
%he change n a quantty called the @i$$s free energy
pro$des a measure of whether a reacton s spontaneous!
%he
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(ow to calculate !G
% l l ti !G
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%alculating !G
i$ilit f ti
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easi$ility of reactions
E$en f Gs post$e at room temperature, there may #e a
hgher temperature at whch a reacton #ecomes feas#le!
"f Ss post$e, there may #e a pont at whch TSs #g
enough to outwegh the enthalpy factor!
G H' TS
post$e
negat$epost$e
negat$e
post$e
post$enegat$e
negat$e
makes TS> H
makes Gmore negat$eno effect Galways post$e
unlkely to make TS > H
yes, a#o$e a
certan temp!
alwaysne$er
usually
H S Bs te"p. increasesC easi$le)
inding the te"perature
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inding the te"perature
8onsder the reducton of alumnum o:de wth car#on
"f G? 0, then T? H@ S
%he temperature at whch ths reacton #ecomes feas#le
can #e calculated! %hs wll #e when G? 0!
=s #othH
andS
are post$e,G
wll #ecome negat$e fTS > H!
H -13 k>"ol'1
Bl2+s,- %+s, 2Bl+s,- %+g,
S -/81>K'1"ol'1
T 2299K
T? 133) @ (1@1000-
&hen is a reaction feasi$le)
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&hen is a reaction feasi$le)
Dolu$ility
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Dolu$ility
"n the same way that reactons are only feas#le f GA 0, a
su#stance wll #e solu#le n water at a specfc temperature
f GsolA 0!
Gsol Hsol' TSsol
post$e
negat$e
post$e
negat$e
post$e
post$e
negat$e
negat$e
Hsol Ssol G feasi$ilityfeas#le f Ts large enough to make
Gnegat$e
always feas#le
ne$er feas#le
usually feas#le Ts unlkely to #e
large enough to make Gpost$e-
Ther"odyna"ics
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Ther"odyna"ics "ol'1
%+s,- 2+g, %2+g,
8onsder the reacton n$ol$ng the com#uston of car#on
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@lossary
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@lossary
&hatFs the keyword)
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&hat s the keyword)
*ultiple choice 5ui:
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*ultipleGchoice 5ui: