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Consider the following half-reactions: A3*(aq) + 3 e' A(s) E° = -0.118 V B2(1) + 2 e →2 B'(aq) E° = -0.956 V a.) Draw a diagram of the voltaic cell created between an A(s) A3*(aq) cell and Pt(s)| B2(1) |B'(aq) cell and a salt bridge of KNO3(aq). Identify: • the half-reaction occurring at the anode • the half-reaction occurring at the cathode • the direction the electrons are flowing through the cell (left to right or right to left) • to which electrode the cations in the salt bridge are flowing · to which electrode the anions in the salt bridge are flowing • whether the concentration of the ion in solution in the anode is increasing, decreasing, or remaining constant • whether the concentration of the ion in solution in the cathode is increasing, decreasing, or remaining constant • whether the solid electrode in the anode is increasing, decreasing, or remaining constant • whether the solid electrode in the cathode is increasing, decreasing, or remaining constant b.) Calculate E°cell for the voltaic cell in (a), in Volts. c.) Write the overall balanced redox reaction occurring in the voltaic cell

Consider the following half-reactions: A3*(aq) + 3 e' A(s) E° = -0.118 V B2(1) + 2 e →2 B'(aq) E° = -0.956 V a.) Draw a diagram of the voltaic cell created between an A(s) A3*(aq) cell and Pt(s)| B2(1) |B'(aq) cell and a salt bridge of KNO3(aq). Identify: • the half-reaction occurring at the anode • the half-reaction occurring at the cathode • the direction the electrons are flowing through the cell (left to right or right to left) • to which electrode the cations in the salt bridge are flowing · to which electrode the anions in the salt bridge are flowing • whether the concentration of the ion in solution in the anode is increasing, decreasing, or remaining constant • whether the concentration of the ion in solution in the cathode is increasing, decreasing, or remaining constant • whether the solid electrode in the anode is increasing, decreasing, or remaining constant • whether the solid electrode in the cathode is increasing, decreasing, or remaining constant b.) Calculate E°cell for the voltaic cell in (a), in Volts. c.) Write the overall balanced redox reaction occurring in the voltaic cell

Chemistry
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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1.) Consider the following half-reactions: A3+(aq) + 3 e - A(s) E° = -0.118 V B2(1) + 2 e → 2 B'(aq) E° = -0.956 V a.) Draw a diagram of the voltaic cell created between an A(s)|A3*(aq) cell and Pt(s)| B2(1) |B'(aq) cell and a salt bridge of KNO3(aq). Identify: · the half-reaction occurring at the anode • the half-reaction occurring at the cathode • the direction the electrons are flowing through the cell (left to right or right to left) . to which electrode the cations in the salt bridge are flowing · to which electrode the anions in the salt bridge are flowing • whether the concentration of the ion in solution in the anode is increasing, decreasing, or remaining constant • whether the concentration of the ion in solution in the cathode is increasing, decreasing, or remaining constant • whether the solid electrode in the anode is increasing, decreasing, or remaining constant whether the solid electrode in the cathode is increasing, decreasing, or remaining constant b.) Calculate E°cell for the voltaic cell in (a), in Volts. c.) Write the overall balanced redox reaction occurring in the voltaic cell
Transcribed Image Text:1.) Consider the following half-reactions: A3+(aq) + 3 e - A(s) E° = -0.118 V B2(1) + 2 e → 2 B'(aq) E° = -0.956 V a.) Draw a diagram of the voltaic cell created between an A(s)|A3*(aq) cell and Pt(s)| B2(1) |B'(aq) cell and a salt bridge of KNO3(aq). Identify: · the half-reaction occurring at the anode • the half-reaction occurring at the cathode • the direction the electrons are flowing through the cell (left to right or right to left) . to which electrode the cations in the salt bridge are flowing · to which electrode the anions in the salt bridge are flowing • whether the concentration of the ion in solution in the anode is increasing, decreasing, or remaining constant • whether the concentration of the ion in solution in the cathode is increasing, decreasing, or remaining constant • whether the solid electrode in the anode is increasing, decreasing, or remaining constant whether the solid electrode in the cathode is increasing, decreasing, or remaining constant b.) Calculate E°cell for the voltaic cell in (a), in Volts. c.) Write the overall balanced redox reaction occurring in the voltaic cell
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