Given the standard reduction potentials: $\mathrm{Fe^{3+} + e^- \rightarrow Fe^{2+}}$ $E^\circ = +0.771$ V and $\mathrm{Cu^{2+} + 2e^- \rightarrow Cu}$ $E^\circ = +0.340$ V. A galvanic cell is set up with a 0.010 M Fe³⁺ solution in the left half‑cell and a 0.010 M Cu²⁺ solution with a copper electrode in the right half‑cell. (a) Write the overall cell reaction, (b) calculate the standard cell potential $E^\circ_{\text{cell}}$, and (c) determine the equilibrium constant $K$ for the cell reaction at 25 °C.

Question

Given the standard reduction potentials: $\mathrm{Fe^{3+} + e^- \rightarrow Fe^{2+}}$ $E^\circ = +0.771$ V and $\mathrm{Cu^{2+} + 2e^- \rightarrow Cu}$ $E^\circ = +0.340$ V. A galvanic cell is set up with a 0.010 M Fe³⁺ solution in the left half‑cell and a 0.010 M Cu²⁺ solution with a copper electrode in the right half‑cell. (a) Write the overall cell reaction, (b) calculate the standard cell potential $E^\circ_{\text{cell}}$, and (c) determine the equilibrium constant $K$ for the cell reaction at 25 °C.

Accepted Answer

Overall: 2 Fe³⁺ + Cu → 2 Fe²⁺ + Cu²⁺; E°cell = 0.431 V; K ≈ 3×10¹⁴

Igcse Model Questions Vol1 2017 Chemistry Question 25

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