2. Using the available materials, design a spontaneous electrochemical cell at standard conditions withinitial E° of +0.90V.a. Label the anode and cathode metalsb. Label the anode and cathode solutionsc. Draw arrows through the wire to indicate the direction of electron flowd. Indicate which ion from the salt bridge will migrate into each chambere. Write the balanced half-reactions for each electrode and the overall balanced equationf. Circle whether each electrode will increase or decrease in massg. Indicate the value of n, the number of electrons/mole rxn, in the balanced equationh. Calculate AG°electronflowKNOanode metalcathode metalanode solution_cathode solutionionmigrationanode half reactioncathode half reactionelectrode mass: increases or decreaseselectrode mass increases or decreasesoverall balanced equation:n=

At anode, oxidation takes place At cathode, reduction takes place Flow of electrons is from anode to…

Answered: 2. Using the available materials,…

2. Using the available materials, design a spontaneous electrochemical cell at standard conditions with initial E° of +0.90V. cell

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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