CHM1046 LECTURE NOTES14.2Equilibrium ReactionDynamic Equilibrium:- The forward and backward reactions are in dynamin equilibrium, meaning they have equal rates14.3The equilibrium constant:K= [C]c[D]d/ [A]a[B]b (products over reactants, and stoichiometry applies)*must have a balanced chemical equation to use this formula since stoichiometry matters- liquids and solids are not considered in the equilibrium constant, K, only gases and aqueous solutions- the significance of the equilibrium constant is seeing whether reactants or products are favored - If given K values for 2 separate reactions, the larger K means products are favored and the smaller K means reactants are favored-If the equilibrium constant is large (larger than unity), that means the equilibrium of the reaction lies far to the right (more products aka much higher concentration onthe product side than on the reactant side)-if K << 1, the reverse (backward) reaction is favored, meaning the reactants are favored-if K is = 1 (or almost equal to 1), then neither (or both) reactions are favored (not one over the other)-if K >> 1, the forward reaction is favored, meaning the products are favored (more products)Kbkwd = 1/ kfwd(so, if you know one of these, take the reciprocal to find the other)- do example 14.2 in the book for
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