question.Salt bridgeA concentration cell similar to the one shown is composed of two Ni electrodes and solutions of different Ni" concentrations. The left compartment contains 0.175M Ni, and the right compartment contains 0.224 M Ni-*Calculate the cell potential for this reaction at 298 K.voltsIn this nickel concentration cell, the reaction would proceed spontaneously

Given: The concentration of Ni2+ in the left compartment = 0.175 M The concentration of Ni2+ in the…

Answered: Salt bridge A concentration cell…

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 85AP

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Similar questions

Give the balanced cell equation and determine for the galvanic cells based on the following half-reactions. Standard reduction potentials are found in Table 17-1. a. Cr2O72+14H++6e2Cr3++7H2OH2O2+2H++2e2H2O b. 2H++2eH2Al3++3eAl
Why would a sacrificial anode made of lithium metal be a bad choice despite its ELi+/Li=2.07V, which appears to be able to protect all the other metals listed in the standard reduction potential table?
Consider a salt bridge voltaic cell represented by the following reaction MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O (a) What is the direction of the electrons in the external circuit? (b) What electrode can be used at the anode? (c) What is the reaction occurring at the cathode?
Determine the overall reaction and its standard cell potential at 25 C for this reaction. Is the reaction spontaneous at standard conditions? Cu(s)|Cu2+(aq)Au3+(aq)|Au(s)
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaueous under each set of conditions at 293.15 K. (a) Hg(l)+S2(aq,0.10M)+2Ag+(aq,0.25M)2Ag(s)+HgS(s) (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half—cell consisting of a nickel electrode in 025 M nickel(l) nitrate solution. (c) The cell made of a half-cell in which 1.0 M aqueous bromide is oxidized to 0.11 M bromine ion and a half-cell in which aluminum ion at 0.023 M is reduced to aluminum metal. Assume the standard reduction potential for Br2(l) is the same as that of Br2(aq).
Using data from Table 18.1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K
Consider the following standard reduction potentials: Tl+(aq)+eTl(s)Ered=0.34VTl3+(aq)+3eTl(s)Ered=0.74VTl3+(aq)+2eTl+(aq)Ered=1.28V and the following abbreviated cell notations: (1) Tl|Tl+Tl3+,Tl+|Pt (2) Tl|Tl3+Tl3+,Tl+|Pt (3) Tl|Tl+Tl3+|Tl (a) Write the overall equation for each cell. (b) Calculate E° for each cell. (c) Calculate G° for each overall equation. (d) Comment on whether G° and/or E° are state properties. (Hint: A state property is path-independent.)

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