A galvanic cell is set up with a copper electrode immersed in 0.10 M $\mathrm{CuSO_4}$ solution and a silver electrode immersed in 0.10 M $\mathrm{AgNO_3}$ solution at 25 °C. Standard reduction potentials: $\mathrm{Cu^{2+}+2e^- \rightarrow Cu(s)}$ $E^\circ = +0.34$ V; $\mathrm{Ag^{+}+e^- \rightarrow Ag(s)}$ $E^\circ = +0.80$ V. (a) Write the overall cell reaction and calculate the standard cell potential $E^\circ_{\text{cell}}$. (b) If the concentrations are changed to $[\mathrm{Cu^{2+}}]=0.10$ M and $[\mathrm{Ag^{+}}]=0.010$ M, calculate the cell potential at 25 °C using the Nernst equation. (c) Is the reaction spontaneous under these conditions?

Question

A galvanic cell is set up with a copper electrode immersed in 0.10 M $\mathrm{CuSO_4}$ solution and a silver electrode immersed in 0.10 M $\mathrm{AgNO_3}$ solution at 25 °C. Standard reduction potentials: $\mathrm{Cu^{2+}+2e^- \rightarrow Cu(s)}$ $E^\circ = +0.34$ V; $\mathrm{Ag^{+}+e^- \rightarrow Ag(s)}$ $E^\circ = +0.80$ V. (a) Write the overall cell reaction and calculate the standard cell potential $E^\circ_{\text{cell}}$. (b) If the concentrations are changed to $[\mathrm{Cu^{2+}}]=0.10$ M and $[\mathrm{Ag^{+}}]=0.010$ M, calculate the cell potential at 25 °C using the Nernst equation. (c) Is the reaction spontaneous under these conditions?

Accepted Answer

Overall reaction: Cu(s) + 2Ag⁺ → Cu²⁺ + 2Ag(s); E°cell = 0.46 V; E (non‑standard) = 0.371 V; reaction is spontaneous (E > 0).

Gce Model Questions Vol1 2022 Chemistry Question 35

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