For the reduction of MnO,¯ to Mn²* in aqueous acid, ɛ° = 1.51 v. For the reduction of I, to 21- in aqueous acid, ɛ° = 0.54 v. 1. Using the above information, balance the whole cell reaction that would occur spontaneously under standard conditions in a galvanic cell and calculate the standard cell potential. a. b. Using KCI, turn the balanced ionic equation from i. into a molecular equation.

For the reduction of MnO,¯ to Mn²* in aqueous acid, ɛ° = 1.51 v. For the reduction of I, to 21- in aqueous acid, ɛ° = 0.54 v. 1. Using the above information, balance the whole cell reaction that would occur spontaneously under standard conditions in a galvanic cell and calculate the standard cell potential. a. b. Using KCI, turn the balanced ionic equation from i. into a molecular equation.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 83AP

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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
The following cell was found to have a potential of 0.124 V: Ag|AgCl(sat’d)||Cu2+ (3.25 10-3 M|mernbrane electrode for Cu2+ When the solution of known copper activity was replaced with an unknown solution, the potential was found to be 0.055 V. What was the pCu of this unknown solution? Neglect the junction potential.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
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Suppose Ered for H+H2 were taken to be 0.300 V instead of 0.000 V. What would be (a) Eox for H2H+ ? (b) Ered for Br2Br ? (c) E for the cell in 34(c)? Compare your answer with that obtained in 34(c).
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