Interactive Activity-The Relationship among E°cell, Keq, and Gibbs Free Energy C

Question

Interactive Activity-The Relationship among E°cell, Keq, and Gibbs Free Energy Constants The following values may be useful when solving this tutorial Constant In an electrochemical cell, the potential difference between two electrodes under standard conditions is known as the standard cell potential (ce). The standard cell potential can be used to identify the overall tendency of a redox reaction to occur spontaneously The spontaneity of a reaction is identified using the Gibbs free energy G . AG is related to E :11. Een1 and Go are also related to equilibrium constant Keq of the reaction. Value 0.337 V 0.257 V Cu R 8.314 J mol1.K-1 96,485 C/mol 298 K Select the image to explore the activity that shows how Ecell, Keq, and are related to each other. Part A eq In the activity, click on the Ecell and Keq quantities to observe how they are related. Use this relation to calculate Ke for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are Cu2+ (aq) + 2e Ca(s) and Ni(s)Ni2+ (aq) + 2e Cift (aq) + Ni(s)-Cu(s) + Ni2+ (aq) The net reaction is Use the given standard reduction potentials in your calculation as appropriate Express your answer numerically to three significant figures. In the activity, you should see a triangle, whose three vertices represent Keq, cell» two vertices and determine the relation between them. You can then reset the activity and select the next two quantities. resent Keq. Ecell, and Go. You can select eq Submit Hints My Answers Give Up Review Part

Explanation / Answer

We will use the relations,

Eocell = Ecathode - Eanode

          = 0.337 - (-0.257)

          = 0.594 V

and,

nFEocell = RTlnKeq

2 x 96485 x 0.594 = 8.314 x 298 lnKeq

Keq = 1.24 x 10^20

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.