Given: Fe (s) + 2 Ag⁺ (aq)→Fe²⁺ (aq) + 2 Ag (s) E ° _cell = 1.24 V What is the standard Gibbs Free-Energy change, D G ° , for this cell reaction?

Question

Quizplus · Accepted Answer

The standard Gibbs Free-Energy change, D G ° , can be calculated using the equation:
D G ° = -nFE °
where n is the number of electrons transferred in the reaction, F is the Faraday constant (96,485 C/mol), and E ° is the standard cell potential. In this case, n = 2 (since 2 electrons are transferred in the reaction), and E ° = 1.24 V. Thus, we have:
D G ° = -2 × 96,485 C/mol × 1.24 V
which simplifies to:
D G ° = -239,195 J/mol
Converting to kJ/mol and rounding to the nearest whole number gives us our final answer of D G ° = -239 kJ/mol (option A).

Given: Fe (S) + 2 Ag+ (Aq)→Fe2+ (Aq) + 2 Ag

Given: Fe (S) + 2 Ag⁺ (Aq)→Fe²⁺ (Aq) + 2 Ag