Sn2+ Sn half cell (E° red = -0.140V) and a standard C12 C1 half cell (E° red = 1.360V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: Sn(s) + The cathode reaction is: Cl2(g) + 2e- The spontaneous cell reaction is: Sn(s) + Cl2(g) The cell voltage is 2.76 V. 2e + Sn2+(aq) 2Cl(aq) + Sn2+(aq) + 2C1-(aq)

Sn2+ Sn half cell (E° red = -0.140V) and a standard C12 C1 half cell (E° red = 1.360V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: Sn(s) + The cathode reaction is: Cl2(g) + 2e- The spontaneous cell reaction is: Sn(s) + Cl2(g) The cell voltage is 2.76 V. 2e + Sn2+(aq) 2Cl(aq) + Sn2+(aq) + 2C1-(aq)

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 133CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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