A galvanic cell is constructed with a copper electrode in 0.010 M Cu²⁺ solution and a silver electrode in 0.010 M Ag⁺ solution. Standard reduction potentials are: Cu²⁺ + 2e⁻ → Cu(s) $E^\circ = +0.34$ V; Ag⁺ + e⁻ → Ag(s) $E^\circ = +0.80$ V. (a) Calculate the standard cell EMF at 25 °C. (b) If the Cu²⁺ concentration is increased to 0.10 M while the Ag⁺ concentration remains 0.010 M, calculate the cell EMF under these conditions and state which electrode acts as the cathode.

Question

A galvanic cell is constructed with a copper electrode in 0.010 M Cu²⁺ solution and a silver electrode in 0.010 M Ag⁺ solution. Standard reduction potentials are: Cu²⁺ + 2e⁻ → Cu(s) $E^\circ = +0.34$ V; Ag⁺ + e⁻ → Ag(s) $E^\circ = +0.80$ V. (a) Calculate the standard cell EMF at 25 °C. (b) If the Cu²⁺ concentration is increased to 0.10 M while the Ag⁺ concentration remains 0.010 M, calculate the cell EMF under these conditions and state which electrode acts as the cathode.

Accepted Answer

(a) 0.46 V; (b) 0.37 V, silver electrode is the cathode

Gce Model Questions Vol1 2023 Chemistry Question 35

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