Lecture 28

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Unformatted text preview: The principle of detailed balance For the reaction A=B in equilibrium we have k1[A] = k ­1[B] or [B]/[A] = k1/k ­1 = KAB, where KAB is the equilibrium constant. Imagine now that we have a system, in which reactions A=B, B=C, C=D, A=C, A=D, … all can take place simultaneously. Let kA→B be the rate of the reaction A → B etc. How can we find the equilibrium concentrations of A, B, C, …? The answer can be deduced from the following statement (the proof of which is beyond the scope of our class): The relations kA→B[A] = kB→A[B] kA→B /kB→A = KAB = exp[ ­(µB0  ­ µA0)/RT] (where KAB is the equilibrium constant of the reaction A=...
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