2. Consider a concentration cell which used the following half-reaction at 273 K. Со2*(ад) + 2е- Со(s) E° = -0.28 V KNO3 salt bridge Cobalt Electrode Cobalt Electrode 1.50 М Со2+ 0.0025 М Со2+ a. Label the anode, cathode, current, anion flow, and cation flow. b. Write a balanced equation for the cell reaction. c. Calculate the cell potential. d. Calculate the equilibrium [Co2+] at the anode and cathode.
2. Consider a concentration cell which used the following half-reaction at 273 K. Со2*(ад) + 2е- Со(s) E° = -0.28 V KNO3 salt bridge Cobalt Electrode Cobalt Electrode 1.50 М Со2+ 0.0025 М Со2+ a. Label the anode, cathode, current, anion flow, and cation flow. b. Write a balanced equation for the cell reaction. c. Calculate the cell potential. d. Calculate the equilibrium [Co2+] at the anode and cathode.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 66QAP: Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C....
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