A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: Cu2 (aq)+Zn () Cu (s)+Zn2(aq) Suppose the cell is prepared with 0.788 MCu2 in one half-cell and 7.32 M Zn2 in the other Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 2
Answers: 3
= -0.7618 V
and anode is ().
![E^{o} - (\frac{2.303 \times RT}{nF}) log {\frac{[Zn^{2+}]}^{1}{[Cu^{2+}]^{1}}](/tpl/images/0550/3152/96c78.png)
![E^{o} - (\frac{2.303 \times RT}{nF}) log {\frac{[Zn^{2+}]}^{1}{[Cu^{2+}]}^{1}](/tpl/images/0550/3152/d6ff2.png)
![E^{o} - (\frac{0.0591}{n}) log \frac{[Zn^{2+}]}^{1}{[Cu^{2+}]}^{1}](/tpl/images/0550/3152/6368f.png)
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