Calculate the standard Gibbs energy for the following cell reaction, A(s) + B ²⁺ (aq) A ²⁺ (aq) + B(s) , if E^ _ cell is 0.556 V .

Step-by-step solution

The given cell reaction is A(s) + B ²⁺ (aq) A ²⁺ (aq) + B(s) . The number of electrons transferred in the reaction is n = 2 . The standard Gibbs free energy change is given by the equation: G^ = -n F E^ _ cell Substituting the given values ( F = 96500 C mol ⁻¹ and E^ _ cell = 0.556 V ): G^ = -2 96500 0.556 G^ = -107308 J mol ⁻¹ G^ -107.31 kJ mol ⁻¹ Answer: -107.31 kJ