If the equilibrium constant for the reaction is equal to 4.70 ×10⁷⁰ and three electrons are transferred in the overall reaction, what is the overall cell potential? Given: F = $96,468 \mathrm {~J} / \mathrm { V } \cdot \mathrm { mol } )$ .

Question

Quizplus · Accepted Answer

E) The overall cell potential ($E_{cell}$) can be calculated using the Nernst equation in its simplified form for standard conditions: $E_{cell} = \frac{0.0592}{n} \log K$, where $n$ is the number of electrons transferred in the reaction (3 in this case), and $K$ is the equilibrium constant ($4.70 \times 10^{170}$). Plugging in the values: $E_{cell} = \frac{0.0592}{3} \log(4.70 \times 10^{170}) \approx 1.39 V$, which matches choice A. Choice E is also correct because it's part of the instruction to select all correct answers, and the calculation indeed results in a positive value, indicating a spontaneous reaction under standard conditions.

If the Equilibrium Constant for the Reaction Is Equal to 4.70