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QUESTION 1: MnO4- <---> MnO2  1.692V         Zn2+ <---> Zn   -0.779V   1. Determine the oxidation numbers of Mn in MnO4- and MnO2.  2. Write the balanced equation (with electrons) for the anodic half cell and cathodic half cell reaction.  3. Write the balanced equation for the complete redox reaction. 4. How many moles(n) are involved in the reaction?  5. What is the cell potiential at standard conditions? 6. Determine the equilibrium constant of the redox reaction at 25C.  7. The concentrations of the ions in the solution are: [Zn2+] = 0.0150 M, [MnO4-] = 0.100 M, and [H+] = 1.00 M. Determine the Q and the cell potiential at 25C.  8. Write the complete cell notation for the cell above. (include metal elctrode and H ions)  Answer question 2

QUESTION 1: MnO4- <---> MnO2  1.692V         Zn2+ <---> Zn   -0.779V   1. Determine the oxidation numbers of Mn in MnO4- and MnO2.  2. Write the balanced equation (with electrons) for the anodic half cell and cathodic half cell reaction.  3. Write the balanced equation for the complete redox reaction. 4. How many moles(n) are involved in the reaction?  5. What is the cell potiential at standard conditions? 6. Determine the equilibrium constant of the redox reaction at 25C.  7. The concentrations of the ions in the solution are: [Zn2+] = 0.0150 M, [MnO4-] = 0.100 M, and [H+] = 1.00 M. Determine the Q and the cell potiential at 25C.  8. Write the complete cell notation for the cell above. (include metal elctrode and H ions)  Answer question 2

Chemistry: Principles and Reactions
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 105QAP: Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a)...
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QUESTION 1: MnO4- <---> MnO2  1.692V         Zn2+ <---> Zn   -0.779V   1. Determine the oxidation numbers of Mn in MnO4- and MnO2.  2. Write the balanced equation (with electrons) for the anodic half cell and cathodic half cell reaction.  3. Write the balanced equation for the complete redox reaction. 4. How many moles(n) are involved in the reaction?  5. What is the cell potiential at standard conditions? 6. Determine the equilibrium constant of the redox reaction at 25C.  7. The concentrations of the ions in the solution are: [Zn2+] = 0.0150 M, [MnO4-] = 0.100 M, and [H+] = 1.00 M. Determine the Q and the cell potiential at 25C.  8. Write the complete cell notation for the cell above. (include metal elctrode and H ions)  Answer question 2
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