Consider the following cell:Cu(s) | CuCl2(0.065 M) || FeCl2(0.035 M) | Fe(s)a) Using the standard reduction potentials table, search for the appropriate half reactions that add to the reaction of this full cell. Whatthe values of the standard potentials of the half cells?E°, =1E°- =Vb) Calculate the standard potential of the full cell.E° =c) Calculate the equilibrium constant of the full cell.K =x 10^d) What is the equilibrium direction of the reaction? Write "a" if the reaction is spontaneous in the forward direction, or "b" if it is nonspontaneous.e) Calculate the potentials of each half cell.E. =VE =f) Calculate the potential of the full cell.E =Vg) What is the direction of the reaction? Write "a" if electrons flow from the Cu electrode to the Fe electrode, or "b" if it is the reverse. A 60.0 mL solution of 0.00750 M OsCl,3- in 1 M HCI was titrated with 0.0300 M IrCI,2- to give OsCl,2- and IrClg3-.a) What is the reducing agent in this reaction? Write "a" for the titrant or "b" for the analyte.b) From the standard potentials table, what is the standard potential of the Os half-reaction?E°, =Vc) What is the standard potential of the Ir half-reaction?E°, =Vd) At what volume of analyte is the equivalence point?Ve =mLe) Calculate the potential (vs. Ag | AGCI) when 10.8 mL of titrant is added.E =Vf) Calculate the potential (vs. Ag | AgCI) at the equivalence point.E =g) Calculate the potential (vs. Ag | AGCI) when 17.6 mL of titrant is added.E =vh) At what volume of analyte will the potential be equal to the standard potential of the Ir half-reaction (ignoring the Ag | AgCl electrode)?V =mL

a) Reduction half cell reaction ( Cathode): Fe2++2e-→Fe Ecell=-0.45 Oxidation half cell reaction…

Consider the following cell: Cu(s) | CuCl2(0.065 M) || FeCl2(0.035 M) | Fe(s) a) Using the standard reduction potentials table, search for the appropriate half reactions that add to the reaction of this full cell. What are the values of the standard potentials of the half cells? E°, = E°. = b) Calculate the standard potential of the full cell. E° = c) Calculate the equilibrium constant of the full cell. K= х 10^

Consider the following cell: Cu(s) | CuCl2(0.065 M) || FeCl2(0.035 M) | Fe(s) a) Using the standard reduction potentials table, search for the appropriate half reactions that add to the reaction of this full cell. What are the values of the standard potentials of the half cells? E°, = E°. = b) Calculate the standard potential of the full cell. E° = c) Calculate the equilibrium constant of the full cell. K= х 10^

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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