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In the cell reaction
$\mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$
$\mathrm{E}_{\text {cell }}^{0}=0.46 \mathrm{~V}$. By doubling the concentration of $\mathrm{Cu}^{2+}, \mathrm{E}_{\text {cell }}^{0}$ is
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$\mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$
$\mathrm{E}_{\text {cell }}^{0}=0.46 \mathrm{~V}$. By doubling the concentration of $\mathrm{Cu}^{2+}, \mathrm{E}_{\text {cell }}^{0}$ is
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decreases by a small fraction
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