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22 Cards in this Set

  • Front
  • Back
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
the value for Keq for a given rxn is constant for a given temp
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 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)