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CHE 132 Lecture Notes - Lecture 36: Nernst Equation, Oxidation State, Equilibrium Constant

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viridianhare340
20 Apr 2019
School
Stony Brook University
Department
Chemistry
Course
CHE 132
Professor
Fernando Raineri

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CHE 132 Lecture Notes - Lecture 35: Standard Hydrogen Electrode, Electrode Potential, Electrochemistry

36

CHE 132 Lecture Notes - Lecture 36: Nernst Equation, Oxidation State, Equilibrium Constant

37

CHE 132 Lecture Notes - Lecture 37: Gibbs Free Energy, Colligative Properties, Strong Electrolyte

Document Summary

Che 132 lecture 33: equilibrium constants, free energy, and nernst. 0 (where n=number of electrons exchanged and f=96485. 3 c / mol: g0 = -rt ln(k) (r is 8. 314 j / k mol) 0 = -( g0 / nf) = (rt / nf) ln(k: so, ecell. If ln(x) = ln(10) x log(x) = 2. 302 x log(x) then we can substitute into the equation above: ecell. / clo3: given the reaction: clo4, e0 (clo4, what is the equilibrium constant for this reaction, we can use the equation k = 10(n e / 0. 0592v) to solve this problem. If you look at the equation, n is the number of electrons transferred; so in this case it would be n=2. You can get this by looking at one half-reaction and seeing the difference in oxidation number: next you will need the e0 value. 0 eanode at the cathode, the cell is being reduced and at the anode it is being oxidized.

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Related Questions

Construct a galvanic (voltaic) cell from the half reactions shown below.Br2 (l) + 2 e- ? 2 Br- (aq) ?o= 1.087 VCu2+ (aq) + 2 e-? Cu (s) ?o= 0.340 VCalculate the equilibrium constant (K) for this cell. Assume that the temperature is 298K.First, consider what happens to the Nernst equation when the system reaches equilibrium:? = ?o - (RT/nF) ln QWhat is ? when the system has reached equilibrium? Is there any driving force left?Remember that ?G = -nF?.At equilibrium, ?G = 0, so ? = 0, too.At equilibrium, Q = K, since all reactants and products are present at their equilibrium concentrations.This simplifies the Nernst equation to:?ocell = [(RT)/nF] ln KNow calculate a value for K.You may need to use scientific notation to record your answer. If so, enter it as: 4E43 which is equivalent to 4x1043

Construct a galvanic (voltaic) cell from the half reactions shown below.Br2 (l) + 2 e- ? 2 Br- (aq) ?o= 1.087 VCu2+ (aq) + 2 e-? Cu (s) ?o= 0.340 VCalculate the equilibrium constant (K) for this cell. Assume that the temperature is 298K.First, consider what happens to the Nernst equation when the system reaches equilibrium:? = ?o - (RT/nF) ln QWhat is ? when the system has reached equilibrium? Is there any driving force left?Remember that ?G = -nF?.At equilibrium, ?G = 0, so ? = 0, too.At equilibrium, Q = K, since all reactants and products are present at their equilibrium concentrations.This simplifies the Nernst equation to:?ocell = [(RT)/nF] ln KNow calculate a value for K.You may need to use scientific notation to record your answer. If so, enter it as: 4E43 which is equivalent to 4x1043