Chemical Equilibrium & LeChatelier's Principle

Chemical Equilibrium & LeChatelier's Principle -...

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Roshni Sheth CH 118-M3 February 17, 2010 Chemical Equilibrium and LeChatelier’s Principle 1. Colors of the Complex Ions 1.) [Co(H 2 O) 6 ] 2+ : hot pink/magenta 2.) [CoCl 4 ] 2- : turquoise/teal 3.) [Cu(H 2 O) 6 ] 2+ : transparent blue 4.) [Cu(NH 3 ) 4 (H 2 O) 2 ] 2+ : dark blue layer at top/transparent blue at bottom 5.) Cu(OH) 2 : colorless with patches of blue precipitate 6.) [CuBr 4 ] 2- : murky blue 2. Addition of Water Since water is included in the complex ions [Co(H 2 O) 6 ] 2+ , [Cu(H 2 O) 6 ] 2+ , and [Cu(NH 3 ) 4 (H 2 O) 2 ] 2+ , its addition would shift the equilibrium of the reaction to be more product-favored. It is not part of the equilibrium constant expression, but it still affects the equilibrium of the reaction because of the complex ions. 3. Temperature Dependence of K Changing the temperature affects the K value because it will affect the way the reactions runs. When the temperature is decreased, the reaction will become more
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Unformatted text preview: reactant-favored. When the temperature is increased, the reaction will become more product-favored. The temperature slightly affected test tubes 1 and 2, so K is less than 0 when the solution is cooled and greater than 0 when the solution is heated. Test tubes 3 and 4 were not affected by the temperature, so K would stay be below 0 regardless of the temperature. 4. Exercise If K is greater than 1, then Gibbs free energy will be positive because the natural log of K will be negative. This means the reaction is reactant favored. If K is less than 1, then Gibbs free energy will be negative because the natural log of K will be positive. This means the reaction is product favored....
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