Cu^{2+} (aq) + Cu (s) → Cu^{2+} (aq) + Cu (s)

↓ E° → oxidation → anode

↑ E° → reduction → cathode

$\overline{){\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{anode}}}}$

E°cell = 0 V

Calculate E_{cell}.

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{-}}{\mathbf{}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}}{\mathbf{n}}\mathbf{\right)}{\mathbf{log}}\frac{\mathbf{\left[}{\mathbf{Cu}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}\mathbf{}\mathbf{anode}}{\mathbf{\left[}{\mathbf{Cu}}^{\mathbf{2}\mathbf{+}}\mathbf{\right]}\mathbf{}\mathbf{cathode}}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{21}\mathbf{=}\mathbf{0}\mathbf{-}\mathbf{}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}}{\mathbf{2}}\mathbf{\right)}\mathbf{log}\frac{\left[{\mathrm{Cu}}^{2+}\right]\mathrm{anode}}{\left[{\mathrm{Cu}}^{2+}\right]\mathrm{cathode}}\phantom{\rule{0ex}{0ex}}\mathbf{}$

[Cu^{2+}] anode must be less than [Cu^{2+}] cathode to have a positive Ecell

A Cu/Cu2+ concentration cell has a voltage of 0.21V at 25 °C. The concentration of Cu2+ in one of the half-cells is 1.6. What is the concentration of Cu2+ in the other half-cell?

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