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Lecture 17 - Outline of Lecture 17 Chemical Equilibria Text...

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Outline of Lecture 17: Chemical Equilibria Text: Atkins Chapter 9 (all) The general form of an equilibrium constant for the reaction: aA + bB = cC + dD is the following expression: K = (activity of C) c (activity of D) d /(activity of A) a (activity of B) b where the activities are determined at equilibrium. If not at equilibrium, then the ratio equals Q. The activity of an ideal gas is its partial pressure. The activity of a compound in a liquid or solution phase is essentially the same as its concentration. The activity of a solid is unity (the number 1). The activity of a nearly pure liquid is also 1. A high activity of a substance means that it is less stable toward reaction These principles are based on the contribution to the entropy that each kind of phase makes to a system. A gas at high pressure has less entropy (per mole) because it is less free. A liquid (or solute) at high concentration has less entropy because there are fewer
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