Consider the following reduction half-reactions: MnO4 (aq) + 8 H*(aq) + 5 e¯ = Mn²+ (aq) + 4H₂O(1) E° = +1.51 V Al³+ (aq) + 3 e 2Al(s) E° = -1.68 V Cl2(g) + 2 e 2 Cl¯(aq) E° = +1.36 V Mg²+ (aq) + 2 e Mg(s) E° = -2.36 V Calculate the standard cell potential for the most spontaneous reaction that can be produced when two of the given half-reactions are combined to form an electrochemical cell. -0.85 V +3.87 V -4.04 V O +2.87 V

Consider the following reduction half-reactions: MnO4 (aq) + 8 H*(aq) + 5 e¯ = Mn²+ (aq) + 4H₂O(1) E° = +1.51 V Al³+ (aq) + 3 e 2Al(s) E° = -1.68 V Cl2(g) + 2 e 2 Cl¯(aq) E° = +1.36 V Mg²+ (aq) + 2 e Mg(s) E° = -2.36 V Calculate the standard cell potential for the most spontaneous reaction that can be produced when two of the given half-reactions are combined to form an electrochemical cell. -0.85 V +3.87 V -4.04 V O +2.87 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe*(aq) + B(s) + 6H,O(1) - Fe(s) + H,BO, (s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reductio Fe3+(aq) + 3 e¯ → Fe(s) E° = -0.04 V H,BO, (s) + 3 H,0*(aq) + 3 e- B(s) + 6 H,O(1) E° = -0.8698 V
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