For the cell involving following reaction. Zn _ ( s ) + Ni _ ( aq ) ⁺² Zn _ ( aq ) ⁺²+ Ni _ ( s ) E _ cell ^ =0.5 ~V . What is standard Gibb's energy change of cell reaction?

Step-by-step solution

The standard Gibbs energy change relates to standard cell potential through the fundamental equation G^ = -nFE^ _ cell , where n represents moles of electrons transferred and F is Faraday's constant, approximately 96500 J/(V mol) . For the redox reaction Zn _ (s) + Ni _ (aq) ⁺² Zn _ (aq) ⁺² + Ni _ (s) , both half-reactions involve two electrons: Zn Zn ²⁺ + 2e^- and Ni ²⁺ + 2e^- Ni , establishing n = 2 . With E^ _ cell = 0.5 V , G^ = -2 96500 0.5 = -96500 J . Converting to kilojoules: G^ = -96.5 kJ , validating opti