LeChatelier's - first prepared the predominant species...

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Juan Robledo CH118-L9 Chemical Equilibrium and LeChatelier’s Principle 1. Colors of the Complex Ions Cobalt(II) Complexes i. Pink [Co(H 2 O) 6 ] 2- ii. Blue [CoCl 4 ] 2+ Copper(II) Complexes iii. Blue [Cu(H 2 O) 6 ] 2+ iv. Dark Blue [Cu(NH 3 ) 4 (H 2 O) 2 ) 2+ v. Blue with precipitate Cu(OH) 2 (s) vi. Green [CuBr 4 ] 2- 2. Addition of Water When water is added to a solution it increases the volume of the solution and thus decreases the concentration being observed. This decrease in concentration causes the equilibrium to shift. In the first test tube HCL was mixed with CoCl 2 6H 2 O. At first the major species was CoCl 4 but when water was added [Co(H 2 O) 6 ] 2+ became the major species. 3. Temperature Dependence of K When the temperature of an exothermic reaction, where heat is a product, is increased the K value will decrease. When the temperature of an endothermic reaction, where heat is a reactant, is increased the K value will increase. When the tube containing the cobalt solution was
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Unformatted text preview: first prepared, the predominant species was [Co(H 2 O) 6 ] 2+ . When the tube was heated to 100°C, the predominant species became CoCl 4 . Juan Robledo CH118-L9 Chemical Equilibrium and LeChatelier’s Principle After the tube was removed from the heat and placed into an ice bath, the predominant species moved back to [Co(H 2 O) 6 ] 2+ . 4. Exercise When a reaction leaves the standard state because of a change in the ratio of the concentrations of the products to the reactants, we have to describe the system in terms of non-standard-state free energies of reaction. The difference between G o and G for a reaction is important. There is only one value of G o for a reaction at a given temperature, but there are an infinite number of possible values of G ....
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