An electrochemical cell consists of a left compartment with a zinc electrode ih contact WILH compartment with a silver electrode in contact with 1.0 mol/L AgNO3(aq). The standard reduction potentials are: E° = 0.80 V Ag* +e = Ag Zn2* + 2e = Zn E° =-0.76 V When this cell is allowed to operate at 25°C, which of the following statements is true? The silver electrode will be the anode. B The concentration of Ag+ ions in right compartment will increase. C) The standard cell potential for this cell is 0.04 V. D The silver electrode will be the cathode. E zn* ions will be reduced to Zn metal.

An electrochemical cell consists of a left compartment with a zinc electrode ih contact WILH compartment with a silver electrode in contact with 1.0 mol/L AgNO3(aq). The standard reduction potentials are: E° = 0.80 V Ag* +e = Ag Zn2* + 2e = Zn E° =-0.76 V When this cell is allowed to operate at 25°C, which of the following statements is true? The silver electrode will be the anode. B The concentration of Ag+ ions in right compartment will increase. C) The standard cell potential for this cell is 0.04 V. D The silver electrode will be the cathode. E zn* ions will be reduced to Zn metal.

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 159MP: A galvanic cell is based on the following half-reactions: In this cell, the copper compartment...

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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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