Electrochemical cells and the voltages they produce arediscussed in sections 19.

Question

Electrochemical cells and the voltages they produce arediscussed in sections 19.4 and 19.5. This question gives youpractice in calculating the voltage of a cell. Note that you arestarting with the overall cell reaction here. Using atable of standard reduction potentials calculate the standard cellpotential (electromotive force) in volts
for the following cell.
2Ag+(aq) + Zn(s) 2Ag(s) + Zn2+(aq)

Explanation / Answer

The half-reactions present (and their standard cell potentials)are: Ag+(aq) + e- => Ag(s) ;Eo = 0.80 V Zn2+(aq) + 2e- => Zn(s) ;Eo = -0.76 V (NOTE: the values forstandard cell potentials are from my textbook. So answersmay vary depending on what your textbook gives for the values. Youmay want to double check.) The equation for standard cell potential is: Eo = Eocathode -Eoanode Since the cathode is the one with the higher cellpotential, we can write Eo = 0.80 - (-0.76)      = 1.56 V

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