Inorganic Exp 5

Inorganic Exp 5 - Experiment #5 Temperature Change and...

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Experiment #5 Temperature Change and Equilibrium Chem 1312 Section: D1 Date Performed: February 15, 2006 Date Due: February 22, 2006 Submission Date: February 22, 2006
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Objective/Introduction: Galvanic cells allow us to harness the electron flow of a chemical reaction that has a positive cell potential. The salt bridge lets the passage of ions in aqueous solution to maintain charge neutrality in each of the half-cells. Half-cells are the two compartments that make up the electrochemical cell. Each half-cell is composed of an electrode, which is dipped in a solution of its respective electrolyte. The Nernst equation was derived from the equation linking free energy changes to the reaction quotient. The Nernst equation gives the electrode potential (E), relative to the standard electrode potential, (E 0 ), of the two half cells. It is known that almost everything is affected by temperature. Historic scientists observed everyday activities and how temperature affects these activities, which led to the formation of the laws of thermodynamics (mathematical forms that explained the observations). The laws of thermodynamics can be used to also explain chemical reactions, which relate the equilibrium condition and the temperature of a reaction. These laws describe chemical reactions with respect to temperature and equilibrium as the change in enthalpy (ΔH°), entropy (ΔS°), and free energy (ΔG°) for the system being observed. By learning the effects of temperature on equilibrium for a reaction, we were able to obtain sufficient information to calculate thermodynamic functions. For this experiment, our group of four constructed an electrochemical cell, which
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This note was uploaded on 02/25/2012 for the course CHEM 4385 taught by Professor Staff during the Fall '11 term at Texas State.

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Inorganic Exp 5 - Experiment #5 Temperature Change and...

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