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

Question

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

The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + 3 I<sub>2</sub>(s) → 2 Al<sup>3+</sup>(aq) + 6 I<sup>-</sup>(aq) The emf generated by the cell when [Al<sup>3+</sup>] = 4.5 × 10<sup>-</sup><sup>3</sup> M and [ ] = 0.15 M is A) 2.20 B) 2.32 C) 2.10 D) 2.39 E) 2.23

] = 0.15 M is The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al(s) + 3 I2(s) → 2 Al3+(aq) + 6 I-(aq) The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [ ] = 0.15 M is A) 2.20 B) 2.32 C) 2.10 D) 2.39 E) 2.23

Quizplus · Accepted Answer

The Nernst equation can be used to calculate the cell potential at non-standard conditions:
Ecell = E°cell - (RT/nF)*ln(Q)
where R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the cell reaction, F is Faraday's constant, and Q is the reaction quotient.
Plugging in the given values:
Ecell = 2.20 - (0.0257/3)*ln((0.15)^6/(4.5*10^-4))
Ecell = 2.32 V (rounded to two significant figures)
Therefore, the answer is B.

The Standard Emf for the Cell Using the Overall Cell