For a galvanic cell, given the following half-reactions and their standard reduction potentials:2CIO3 +12H+10eCl₂ + 6H2O E°= +1.51 voltS2₂082 +2e2SO4²-Eº = +2.05 voltCalculate the value of the equilibrium constant, Kc.Report your answer in scientific notation with 1 place past the decimal point.Use this format: 1.2*10^3Type your answer...

The relation between Eocell and equilibrium constant is given as follows;logK=nEo0.0591 ----(1)

For a galvanic cell, given the following half-reactions and their standard reduction potentials: 2CIO3 +12H+ +10eCl₂ + 6H2O E°= +1.51 volt E = +2.05 volt S₂082 +2e2SO42- Calculate the value of the equilibrium constant, Kc. Report your answer in scientific notation with 1 place past the decimal point. Use this format: 1.2*10^3

For a galvanic cell, given the following half-reactions and their standard reduction potentials: 2CIO3 +12H+ +10eCl₂ + 6H2O E°= +1.51 volt E = +2.05 volt S₂082 +2e2SO42- Calculate the value of the equilibrium constant, Kc. Report your answer in scientific notation with 1 place past the decimal point. Use this format: 1.2*10^3

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 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the standard potential...

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a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
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The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).

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