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22 Cards in this Set
- Front
- Back
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Why are solids and liquids not included in equilibrium calculations
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b/c their concentrations dont change. Also, for this reason, we can omit solvents in dilute solutions
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Unit of measurement when dealing with gases
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partial pressures (which are equal to the concentration)
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Two chemical states that are used in calculating equilibrium
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1. aqueous dissolved particles
2. Gases |
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t/f
the value for Keq for a given rxn is constant for a given temp |
t
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Keq < 1
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rxn favors reactants
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Keq = 1
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neither products nor reactants are favored
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Keq > 1
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rxn favors products
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Compare Reaction Quotient to Keq
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Q is the same rate as Keq, but it is for a rxn that has not yet reached equilibrium
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Q < Keq
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rxn proceeds in a forward direction
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Q = Keq
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rxn is at equilibrium
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Q > Keq
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rxn proceeds in reverse direction
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The relationship of the reaction quotient to Keq is the basis of what principle
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LeChatlier's principle
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Le Chatlier's Principle
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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 |
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Molar Solubility
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number of moles of a salt that will saturate a liter of H2O
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Qsp < Ksp
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more salt can be dissolved
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Qsp = Ksp
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solution saturated
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Qsp > Ksp
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excess salt will precipitate
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Common Ion effect
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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)
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Ksp for MX3
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Ksp=27x^4
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Ksp for MX2
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Ksp= 4x^3
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Ksp for MX1
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Ksp= x^2
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General solubility rule for slightly soluble salts
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MXn, Ksp= n^(n)x^(n+1)
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