Lecture 28

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

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=...
View Full Document

Ask a homework question - tutors are online