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Lecture 1 - Kinetic Theory of Gases

# Lecture 1 - Kinetic Theory of Gases - Thermodynamics vs...

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Thermodynamics vs Kinetics Chemical Reaction or Biological Process: K eq = [B]/[A] = k f /k rev (Thermo, 107A) k f = forward rate constant (Kinetics, 107B) A B k f k rev Thermo predicts how far a rxn proceeds (K eq ). State function depends on difference between final & initial state ( G°). Kinetics measures how fast (k f in seconds or millenia). Rate depends on barrier and details of pathway . K eq = [B]/[A] exp(- Gº/RT) k f exp(-E a /RT) C(s) diamond C(s) coal B A Time Conc A B E a A B k f k rev Free Energy K eq ~ 10 4 1/k f ~ 1000 yrs Glycolysis (glucose pyruvate + NADH) Protein phosphorylation (R + ATP R-P + ADP) Dephosphorylation (R-P + H 2 O R + P i ) Rxn coordinate

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Kinetic Theory of Gases (Ch 2.6-2.9) Ch 2 Homework Problems : 52, 54, 56, 58, 62, 64, 68, 78, 98, 100 Why study gases? Gas properties (pressure or volume) relate to speed of moving molecules (hence, kinetics). Gas properties are easy to measure (PV = nRT). Gas reaction kinetics modeled by molecular collisions: A B rate (# of collisions) X (collision speed) Kinetics of ideal gas generalize to kinetics of biological reactions in dilute solution (i.e. ideal soln: <10 -3 M).