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Lecture 6

CHEM 1A03 LECTURE 6 OCTOBER 8-14.docx

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Department
Chemistry
Course
CHEM 1AA3
Professor
David Brock
Semester
Spring

Description
CHEM 1A03 LECTURE 6 – DYNAMIC CHEMICALEQUILIBRIUM October 9-14 2012 Equilibrium Constant (K) K is a thermodynamic parameter characterizing the tendency for a chemical rxn or process to occur. Chemical process are reversible – the extent of rxn is determined by L K is a ratio of product to reactant ACTIVITIES (a) – effective concentration or pressure – at llbm. The form of K depends on the balanced chemical equation: [PRODUCTS] K = [REACTANTS] to the powers of their respective numerical coefficients Activity The activity (a) of a solute S is given by a = y[S]/[S]o • where [S] o 1mol/L is the reference state. • Y is the activity coefficient; assume y=1 (it is under “ideal conditions” – conc < 0.001M) The activity (a) of a gas G is given by a = y*P /g o • Use a = P (go units) where P = 1otm is the reference state; assume y=1 The activity (a) of a pure solid of liquid is 1 – This means you can ignore them when setting up the equilibrium constant Different Constants Reserve the subscript on K to denote the type of rxn. K expression MAY include concentrations (aw) and/or pressures (gases) K spdissolution rxns K – cctivities are concentrations K – acpivities are partial pressures. Reaction Quotient (Q) K = ratio of products/reactants at llbm (constant at a given temperature) Q = ratio of products to reactants at ANY INSTANT (can hold any balue) If Q < K  Reaction proceeds forwards If Q > K  Reaction moves backwards If Q = K  llbm is established. Octanol Water Partition coefficient K owis the octanol-water partition coefficient and gives a measure of lipophilicity of a solute (S) molecule. If a beaker has water
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