termodinámica química 2016
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TERMODINÁMICA QUÍMICA
José Ángel Rojas Zamorano
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A + ! +
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A + ! + "
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∆# $e %na rea&&'(n
é es le ∆#
é nos ,erm'-e sa.er so.re el ,ro&e$er $e %na rea&
mo se &al&%la
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2
33
∆H Entalpia De Reacción (kJ/mol)
(- 393.5) (- 285.8)(0)(-277) -
+
+
-
1 3
2
3
= +277 - 787 - 857.4
∆H
= - 1367.4
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2 33
∆! E"#R$%&' (J/mol)
(+213.74) (69.95)(+205.07)(+161.04)-
+
+
-
1 3 2 3
-161.04 +427.48 +209.55-617.21
∆! = -141. J/6/17/16 09:58:38 PM 7
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2 33
∆*! E"ER*&' &,RE DE *&,, (J/mol)
(-394.4) (-237.13)(o)(-174.2)1 3 2 3- + +-+174.2 - 788.8
∆*! = -13. J
0 - 711.39
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1 J 1!!!J
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Cálculo de H0 a partir deEntalpía de !or"aci#n
Nor"ale
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)*%é es %na Rea&&'(n $e orma&'(n
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Para %narea&&'(n:
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ecuaci#n de $irc%%o& H ' H(T)
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0
P
Para %narea&&'(n:
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Si Cp = Cp(T)
Si Cp = Constante
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Si Cp = Cp(T)
Si Cp = Constante
' se -oma $e re4eren&'a las &on$'&'ones normales
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' $
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a s's-emas $e %n &om,onen-e
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e $e ess
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!o&'en-e $e Rea&&'(n
é es * (!o&'en-e $e Rea&&'(n
é nos ,erm'-e sa.er so.re el ,ro&e$er $e %na rea&
mo se &al&%la
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Q < K Q > K
0 Q = K Q
Espontáneo No Espontáneo
Eq!"!#$!o
'n'&'o $e la rea&&'(n * 0
a rea&&'(n aan;a en -an-o * < =
a rea&&'(n se$e-'ene &%an$o * =
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E0ili2io
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E0ili2io
'ance e
2eacción
2eactio5
p2o0cto5
=
= ! = 6/17/16 09:58:39 PM 3
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Reacci#nEpontán
ea
Reacci#n
NoEpontánea
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*+O* (,) - O*(,) *+O
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