CH 118 lechateliers equilibrium

CH 118 lechateliers equilibrium - exothermic reactions...

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CH 118 Chemical Equilibrium and LeChatelier’s Principle I. Color of Complex Ions Pink -> [Co(H 2 O) 6 ] 2+ Blue -> [CoCl 4 ] 2- Blue -> [Cu(H 2 O) 6 ] 2+ Blue -> [Cu(NH 3 )4(H 2 O) 2 ] 2+ Blue -> Cu(OH) 2 Blue -> [CuBr 4 ] 2- II. Addition of Water Water is not included in the equilibrium constant expression because the concentration of it cannot change as the reaction occurs. However, adding water can decrease the concentration of the reactant and cause a shift towards the left. For example, the addition of water to CuBr 2 caused the color to go from green to blue. Also, the reaction between [Co(H 2 O) 6 ] 2+ and HCl was blue (product favored), but when water was added it turned purple (shifting left and almost at equilibrium). III. Temperature Dependence of K The value of K can be different for the same reaction at different temperatures. For example,
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Unformatted text preview: exothermic reactions favor the products. Also, reactions can occur faster at higher temperatures than lower temperatures. Therefore, it is important to note the temperature for each K value. Test tube #1 was purple (K = 1) at room temperature, blue (K >> 1) at 100 C, and pink (K <<1) at 0 o C. Test tubes #2, 3, and 4 all remained pink (K << 1) at all three temperatures. IV. Gibbs Free Energy Exercise The relationship between Gibbs free energy and equilibrium constant is ∆G = -RT ln K If K is much greater than 1, then ∆G is negative, indicating a product-favored reaction. If K is much less than 1, then ∆G is positive, indicating a reactant-favored reaction....
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CH 118 lechateliers equilibrium - exothermic reactions...

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