Use the standard half-cell potentials listed below to calculate the standard cel

Question

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25C. (The equation is balanced.)

Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s)

Sn2+(aq) + 2 e- ? Sn(s) E = -0.14 V
Ag+(aq) + e- ? Ag(s) E = +0.80 V

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25C. (The equation is balanced.)

Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s)

Sn2+(aq) + 2 e- ? Sn(s) E = -0.14 V
Ag+(aq) + e- ? Ag(s) E = +0.80 V

Explanation / Answer

For the given reaction -

Sn(s) + 2 Ag+(aq) ------> Sn2+(aq) + 2 Ag(s)

oxidation Half reaction: Sn (s) --------> Sn2+ (aq) + 2e-         ; Eoxi0 = 0.14 V

reduction half reaction: 2 Ag+ (aq) + 2e- -----> 2 Ag (s)      ; E0red = 0.80 V

Thus -

           Ecell0 = 0.80 V + 0.14 V = 0.94 V (option D)

The standard cell potenial, Ecell0 = Ered0 + E0oxi

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