The standard cell potential (E°_cell)of the reaction below is -0.55 V. The value of ΔG° for the reaction is ________ J/mol. I₂ (s) + 2Br^- (aq) → 2I^- (aq) + Br₂ (l) A)0.54 B)0.55 C)5.5 × 10^-6 D)1.1 × 10⁵ E)none of the above

Question

Quizplus · Accepted Answer

The relationship between standard cell potential and standard free energy change is given by the equation ΔG° = -nFE°, where n is the number of electrons transferred and F is the Faraday constant (96,485 C/mol). In this case, n = 2 (since 2 electrons are transferred in the balanced equation) and E° = -0.55 V. Substituting these values into the equation gives:

ΔG° = -nFE°
ΔG° = -(2)(96,485 C/mol)(-0.55 V)
ΔG° = 1.06 × 10^5 J/mol

Rounding to two significant figures, the value of ΔG° is 1.1 × 10^5 J/mol, which corresponds to answer choice D.

The Standard Cell Potential (E°cell)of the Reaction Below Is -0

The Standard Cell Potential (E°_cell)of the Reaction Below Is -0