The standard emf for the cell using the overall cell reaction below is +2.20 V: 2Al (s) + 3I₂ (s) → 2Al³⁺ (aq) + 6I^- (aq)
The emf generated by the cell when [Al³⁺] = 4.5 × 10^-3 M and [I^-] = 0.15 M is ________ V.

Question

Quizplus · Accepted Answer

To solve the problem, we can use the Nernst equation: E = E° - (RT/nF) × ln(Q) where: E° = standard emf = +2.20 V R = gas constant = 8.314 J/mol·K T = temperature in Kelvin n = moles of electrons transferred in the balanced equation (in this case, n = 6) F = Faraday's constant = 96,485 C/mol Q = reaction quotient = [Al³⁺]²/[I^-]³ Substituting the given values, we get: E = 2.20 - (8.314 × 298/6 × 96,485) × ln[(4.5 × 10⁻¹³)²/(0.15)³] E = 2.32 V Therefore, the answer is B) 2.32.

The Standard Emf for the Cell Using the Overall Cell