chem ec - endothermic K increases with increasing...

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Yash Jhala Brittland-465 Extra Credit 1. The forward reaction in the equations is Endothermic. Since the equation has a reactant that contains a lot higher exponent [Cl^4], the K will be very small. Due to that, the reaction is endothermic and product favored Eq 1: [Co(H 2 O) 6 ] 2+ (aq) + 4Cl - (aq)  [CoCl 4 ] 2- + 6 H 2 O (l) Eq 2: [Cu(H 2 O) 6 ] 2+ (aq) + 4Cl - (aq)  [CuCl 4 ] 2- + 6 H 2 O (l) 2. Delta G is Gibbs free energy, which defines the total energy gained or lost during the reaction. This is the only factor that can change the K constant along with temperature. According to the equation, when the reaction is exothermic (Δ H o is negative), then K decreases with increasing temperature. If the reaction is
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Unformatted text preview: endothermic, K increases with increasing temperature. This also coincides with LeChatelier’s Principle. Therefore, if K is greater than 1, then Delta G is negative, the reaction is exothermic, favoring the making of reactants. If K is less than 1, Delta G is positive, and the reaction is endothermic, favoring the making of products. As K goes up, we can determine that the Delta G will go down, therefore making the reaction more product favored. As K goes down, we can determine that Delta G goes up, therefore making the reaction more reactant favored....
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This note was uploaded on 03/27/2008 for the course CHEM 103 taught by Professor Wendt during the Fall '07 term at University of Wisconsin.

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