07 Question Consider the following standard reduction potentials. O₂(g) +2H₂O(1)-4e-40H (aq) E-0.401 V Ca²+ (aq) +2e Ca(s) E-2.868 V Part 1 Write the balanced chemical equation that occurs in an electrochemical cell that employs these half-reactions. Include states of matter. XX ( 8. 2Ca(s) + O₂(g) + 4H (aq) → 2Ca² (aq) + 2H₂O(aq) Part 3 Calculate the maximum amount of work produced by the cell when the partial pressure of O₂ is 0.1950 atm, the pH is 7.122, and the concentration of Ca2* is 0.0130 M. -2153.49 kj

07 Question Consider the following standard reduction potentials. O₂(g) +2H₂O(1)-4e-40H (aq) E-0.401 V Ca²+ (aq) +2e Ca(s) E-2.868 V Part 1 Write the balanced chemical equation that occurs in an electrochemical cell that employs these half-reactions. Include states of matter. XX ( 8. 2Ca(s) + O₂(g) + 4H (aq) → 2Ca² (aq) + 2H₂O(aq) Part 3 Calculate the maximum amount of work produced by the cell when the partial pressure of O₂ is 0.1950 atm, the pH is 7.122, and the concentration of Ca2* is 0.0130 M. -2153.49 kj

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.47QE

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Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
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The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
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