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1.) Given the following notation for an electrochemical cell          Pt(s) | H2(g) | H+(aq) || Ag+(aq)...

1.) Given the following notation for an electrochemical cell

         Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s),

what is the balanced overall (net) cell reaction?  

A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq
B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s)
C.  H2(g) + Ag+(aq) ®  H+(aq) + Ag(s
D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq)
E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s)

2.) Calculate E°cell for the following (nonspontaneous) reaction:


        Cd(s) + 2Fe3+(aq)  ®  2Fe2+(aq) + Cd2+(aq) →

A. -0.37 V
B. + 0.37 V
C. -1.17 V
D. + 1.17 V
E. none of the answers provided is correct
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Answer #1

1)


Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s),

       anode                   cathode

at anode : oxidation

     H2(g) ----> 2H^+(aq) + 2e-

at cathode : reduction

    2Ag^+(aq) + 2e-   ----> 2 Ag(S)

overall reaction :

H2(g) ----> 2H^+(aq) + 2e-

2Ag^+(aq) + 2e-   ----> 2 Ag(S)

------------------------------------
H2(g) + 2Ag^+(aq) -----> 2H^+(aq) + 2 Ag(S)

------------------------------------------

answer: B

2)


E0cell = E0cathode - E0anode

E0cathode = E0Fe^3+/Fe^2+ = 0.77 V

E0anode = E0Cd^2+/Cd = -0.4 V

      = 0.77 - (-0.4)

   = 1.17 v

answer: D

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