The standard cell potential is +0.460 V for the following electrochemical cell reaction: Cus) + 2Ag⁺aq) $\rightarrow$ Cu²⁺aq) + 2Ags). What is the ∆G°_rxn?

Question

Quizplus · Accepted Answer

The Gibbs free energy change (∆G°) for a reaction can be calculated using the formula ∆G° = -nFE°cell, where n is the number of moles of electrons transferred in the reaction (which is 2 for this reaction), F is the Faraday constant (96485 C/mol), and E°cell is the standard cell potential (0.460 V). Plugging in the values gives ∆G° = -2 * 96485 C/mol * 0.460 V = -88.8 kJ/mol (using the conversion 1 J = 1 C*V and the fact that 1000 J = 1 kJ).

The Standard Cell Potential Is +0 →\rightarrow→ Cu2+aq) + 2Ags)

The Standard Cell Potential Is +0 $\rightarrow$ Cu²⁺aq) + 2Ags)