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### 22 Cards in this Set

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 Why are solids and liquids not included in equilibrium calculations b/c their concentrations dont change. Also, for this reason, we can omit solvents in dilute solutions Unit of measurement when dealing with gases partial pressures (which are equal to the concentration) Two chemical states that are used in calculating equilibrium 1. aqueous dissolved particles 2. Gases t/f the value for Keq for a given rxn is constant for a given temp t Keq < 1 rxn favors reactants Keq = 1 neither products nor reactants are favored Keq > 1 rxn favors products Compare Reaction Quotient to Keq Q is the same rate as Keq, but it is for a rxn that has not yet reached equilibrium Q < Keq rxn proceeds in a forward direction Q = Keq rxn is at equilibrium Q > Keq rxn proceeds in reverse direction The relationship of the reaction quotient to Keq is the basis of what principle LeChatlier's principle Le Chatlier's Principle 1. rxn is always trying to get to equilibrium 2. adding/ removing products or reactants pushes the rxn to favor that side, in order to compensate 3. heat is considered a product or reactant for exo/endotherm rxns, rsp. 4. inert gases and catlysts have not affect on this principle Molar Solubility number of moles of a salt that will saturate a liter of H2O Qsp < Ksp more salt can be dissolved Qsp = Ksp solution saturated Qsp > Ksp excess salt will precipitate Common Ion effect A secondary rxn's reactants or products can effect whether another rxn favors the product or reactant side if the two equations share one or more ions in common (due to LCP) Ksp for MX3 Ksp=27x^4 Ksp for MX2 Ksp= 4x^3 Ksp for MX1 Ksp= x^2 General solubility rule for slightly soluble salts MXn, Ksp= n^(n)x^(n+1)