➤ The cell potential for the Daniel cell is 1.10 V at 298 K under standard conditions. Calculate equilibrium constant. Ans. 1.6 x 1037 ➤Use standard reduction potentials to calculate the standard Gibbs free energy at 298 K for the reaction Ans. -2.90 KJ mol-1 Fe2+ + Ag+ (aq) →Fe3+, (aq) + Ag(s) (aq) ►Consider the cell, Al (s) | Al³+ || Au³+ | Au (s) a. At which electrode does reduction occur? b. Which electrode is the anode? c. Which substance is acting as reducing agent? d. Write half reaction for the two half cell? e. To which electrode will cations migrate?

➤ The cell potential for the Daniel cell is 1.10 V at 298 K under standard conditions. Calculate equilibrium constant. Ans. 1.6 x 1037 ➤Use standard reduction potentials to calculate the standard Gibbs free energy at 298 K for the reaction Ans. -2.90 KJ mol-1 Fe2+ + Ag+ (aq) →Fe3+, (aq) + Ag(s) (aq) ►Consider the cell, Al (s) | Al³+ || Au³+ | Au (s) a. At which electrode does reduction occur? b. Which electrode is the anode? c. Which substance is acting as reducing agent? d. Write half reaction for the two half cell? e. To which electrode will cations migrate?

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 3P

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