Question
In a copper-silver cell, why must the $\mathrm{Cu}^{2+}$ and $\mathrm{Ag}^{+}$ solutions be kept in separate containers?
Step 1
These ions are in solution and are associated with their respective metal electrodes. Show more…
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For the redox reaction $\mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+}(\mathrm{aq})$, why can't you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing $\mathrm{CuCl}_{2}(\mathrm{aq})$ and $\mathrm{ZnCl}_{2}(\mathrm{aq})$ ?
For the reaction $\mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+}(\mathrm{aq})$, why can't you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing $\mathrm{CuCl}_{2}(\mathrm{aq})$ and $\mathrm{ZnCl}_{2}(\mathrm{aq}) ?$
For the reaction $\mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+}(\mathrm{aq})$ why can't you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing $\mathrm{CuCl}_{2}(\mathrm{aq})$ and $\mathrm{ZnCl}_{2}(\mathrm{aq})$ ?
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