Problem: Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 degrees C. Sn(s) │ Sn2+ (aq, 0.022M) ║ Ag+ (aq, 2.7M) │Ag(s)   Sn2++ 2e–→ Sn(s)  E◦cell = – 0.14   Ag+ + 1e– → Ag(s) E◦cell = 0.8 A. -0.83 V B. +1.31 V C. -0.66 V D. +1.01 V E. +0.01 V

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 degrees C.

Sn(s) │ Sn2+ (aq, 0.022M) Ag+ (aq, 2.7M) │Ag(s)

Sn2++ 2e→ Sn(s)  Ecell = – 0.14

Ag+ + 1e→ Ag(s) Ecell = 0.8

A. -0.83 V

B. +1.31 V

C. -0.66 V

D. +1.01 V

E. +0.01 V

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