Kelvi

For a cell involving one electron $E^\circ_{cell} = 0.59$ V at $298$ K, the equilibrium constant for the cell reaction is:

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Electrochemistry

2019

chemistry

$1.0 \times 10^2$

$1.0 \times 10^5$

$1.0 \times 10^{10}$

Explanation

To solve this problem, we will use the Nernst equation at equilibrium. $\\$ At equilibrium, the cell potential $E_{cell}$ is zero, and the Nernst equation is given by: $\\ E_{cell} = E^\circ_{cell} - \frac{RT}{nF} \ln K \\$

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For a cell involving one electron Ecell∘=0.59 E^\circ_{cell} = 0.59 Ecell∘​=0.59 V at 298 298 298 K, the equilibrium constant for the cell reaction is:

Explanation

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For a cell involving one electron $E^\circ_{cell} = 0.59$ V at $298$ K, the equilibrium constant for the cell reaction is: