TERMODINAMIKA, BIOENERGETIKA
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1 TERMODINAMIKA, BIOENERGETIKA Osnovni termodinamski koncepti Fizikalni pomen termodinamskih količin ph in standardni pogoji Sklopljeni procesi Energijsko bogate biomolekule Osnovni termodinamski koncepti Sistem: del celote, ki ga obravnavamo (vprašanje kriterijev za določitev sistema, struktura sistema, dinamika sistema) Okolje: vse izven sistema Izolirani sistem ne izmenjuje z okoljem snovi ali energije Zaprti sistem izmenjuje samo energijo Odprti sistem izmenjuje tako snovi kot energijo Sistem opišemo s termodinamskimi spremenljivkami T, p, V, n Glavne termodinamske funkcije so entalpija, entropija in prosta energija Toplota, q Toplota, q Snov, m Okolje Okolje Okolje 1
2 1.zakon termodinamike Celotna energija izoliranega sistema je konstantna! U (ali E) je notranja energija kinetična in potencialna energija omogoča prenos toplote in opravlja delo U je neodvisna od poti (funkcija stanja) U 2 -U 1 = Δ U = q w (-w: iz sistema v okolje!) q je toplota, absorbirana v sistem iz okolja w je delo, ki ga opravi sistem na okolje (npr. tenzijska sila mišičnega vlakna) U je enaka izmenjani toploti pri konst. V Eksotermni procesi- ko se toplota sprošča Endotermni procesi- ko sistem privzema toploto ENTALPIJA- H Funkcija pri konst. p Definicija: H = U + p.v ΔH = ΔU + p.δv (1) ΔH je toplota q absorbirana pri konst. p Volumen V je ~ konst. v biokemijskih sistemih (raztopinah) Velja tudi: w = p.δv + w (2) (w =drugo delo) Iz (1) in (2) ΔH= ΔU + p.δv = q p w + p.δv = = q p (p.δv + w ) + p.δv = q p w Če w ~ 0 (pri npr. kemijskih reakcijah) UΔ ~ ΔH ~ q p ΔH >0 endotermna toplota se porablja (npr. razpad vezi) ΔH <0 eksotermna toplota se sprošča (npr. tvorba vezi) 2
3 2.zakon termodinamike Sistemi stremijo k neredu! Sistemi težijo od urejenega proti neurejenemu stanju (npr. število ekvivalentnih načinov kako uredimo komponente sistema) L. Boltzmann 1877: S = k B.lnW k B =Boltzmannova konst., W=število vseh možnih stanj sistema ENTROPIJA- S Mera za neurejenost stanja Urejeno stanje: majhna entropija Neurejeno stanje: velika entropija R. Clausius, 1864: Pri T = konst. Spontani, ireverzibilni proces: ds irev. dq/t (T=absolutna T pri kateri pride do spremembe) Sistem v ravnotežju med procesom (reverzibilni): ds rev. = dq/t Pri konst. T (tipični za biološke procese) ΔS q/t 3
4 3.zakon termodinamike Entropija popolnoma urejene snovi pri temperaturi absolutne ničle je 0 Entropija popolnoma urejene snovi se bliža vrednosti 0 J/K, če T 0K Pri T = 0 K S = 0 J/K Za proces pri p = konst. velja: C p = ΔH/ΔT C p je toplotna kapaciteta pri konst. p GIBBSOVA PROSTA ENERGIJA- G Gibbs, 1878 ; Hipotetična, vendar koristna količina omogoča oceniti spontanost reakcije (smer reakcije) G je funkcija stanja sistema aditivna G = H T.S Za vsak proces pri p, V = konst. velja: ΔG = ΔH T.ΔS = q -T.ΔS Če ΔG = 0, je reakcija v kem. Ravnotežju; če ΔG < 0, je reakcija spontana (poteka, kot je napisana; dogovor: L D strani) Eksergoni procesi ΔG < 0 Endergoni procesi ΔG > 0 4
5 Sprememba proste energije ΔG in standardne proste energije ΔG o Standardni pogoji T=25 o C, ph=7, 1 atm (=101, 3 kpa), 1M koncentracije oznake: ΔG o, ΔH o, ΔS o Biokemijski standardni pogoji [H + ] = 10-7 M ph = 7,0; [H 2 O] = 55,5 M Oznake: ΔG o, ΔH o, ΔS o Za poljubno reakcijo: aa + bb cc + dd velja: ΔG = ΔG 0 ' + c [ C].[ D] R. T.ln a b [ A].[ B] Pri kemijskem ravnotežju velja: a) ΔG = 0 in b) K r =([C r ] c.[d r ] d /[A r ] a.[b r ] b ) 0 = ΔG o + RT ln K r ΔG o = - RT ln K r d 5
6 Zveza med K r in T (van t Hoff) van t Hoffova enačba omogoča določitev temodinamskih količin ΔH in ΔS Če velja: ΔG 0 =ΔH 0 -T. ΔS 0 in ΔG 0 = -RT ln K r -RT ln K r =ΔH 0 -T. ΔS 0 ln Kr ΔH = R 0 1. T + ΔS R 0 6
7 van t Hoffov graf, K r = f(1/t) 0 ΔH 1 ΔS ln Kr =. + R T R y = a. x + b Naklon = ΔH 0 R 0 Kalorimeter merjenje q p (q p ~ ΔH) 7
8 O'Brien R & Haq I (2004) Applications of Biocalorimetry: Binding, Stability and Enzyme Kinetics. In Biocalorimetry 2 (Ladbury JE & Doyle M, eds.). ITC Isothermal titration calorimetry DSC Differential scanning calorimetry O'Brien R & Haq I (2004) Applications of Biocalorimetry: Binding, Stability and Enzyme Kinetics. In Biocalorimetry 2 (Ladbury JE & Doyle M, eds.). 8
9 Prenos energije v bioloških sistemih Problem endergonih reakcij Snovi, ki so kemijsko nestabilne njihov razpad (hidroliza) je zelo eksergon (eksotermen), spontan ΔG0 << 0! Sodelovanje dvoje vrst biomolekul: Reducirani koencimi (NADPH, FADH 2 ) Energetsko bogate spojine (npr. fosfati) Energijsko sklopljene reakcije V biol.sistemih je endergona reakcija mogoča, če je energijsko sklopljena z eksergono! Splošni primer: ΔG 0 A+B C+D + 50 kj/mol C+F G - 70 kj/mol Σ A+B+F D+G - 20 kj/mol 9
10 Sklopljene reakcije, ki vključujejo ATP Fosforilacije glukoze, nastane glukoza-6-fosfat in ADP. Energijsko bogate molekule - primeri Standardna prosta energija fosfatnih skupin nekaterih biološko pomembnih spojin 10
11 Kemijska narava energijsko bogatih snovi Kemijsko nestabilne spojine nestabilna vez, velik potencial za oddajo skupine Kemijska delitev: fosfoanhidridi (ATP, PPi, itd.) fosfo-acilni anhidridi (Acetilfosfat, 1,3-BFG) enol-fosfati (PEP) gvanidino-fosfati (kreatinfosfat, fosfoarginin) Stabilizacija produktov pri hidrolizi zmanjšanje elektrostatskega odboja (ATP) ionizacija (ATP, 1,3-BPG, acetilcoa) tautomerija (fosfoenolpiruvat) resonančna stabilizacija (ATP, 1,3-BFG, fosfokreatin, acetil CoA) Resonančna in elektrostatska stabilizacija fosfoanhidridov in hidrolitskih produktov 11
12 Hidroliza fosfoenolpiruvata Resonančna stabilizacija fosfogvanidinov 12
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