Which from following equations represents a correct relationship between standard cell potential and…

Which from following equations represents a correct relationship between standard cell potential and equilibrium constant for cell reaction?
  1. $\mathrm{E}_{\mathrm{cell}}^{\circ}=-\frac{2.303 \mathrm{RT}}{\mathrm{nF}}$
  2. $\mathrm{E}_{\text {cell }}^{\circ}=\frac{0.0592}{\mathrm{nF}} \log _{10} \mathrm{~K}$
  3. $\mathrm{E}_{\text {cell }}^{\circ}=\frac{0.0592}{\mathrm{n}} \log _{10} \mathrm{~K}$
  4. $\mathrm{E}_{\text {cell }}^{\circ}=\frac{0.0592}{\mathrm{n}} \ln \mathrm{K}$

Solution

The correct equation that represents the relationship between the standard cell potential and the equilibrium constant for the cell reaction is: (3) $E_{\text {cell }}^{\circ}=\frac{0.0592}{n} \log _{10}(K)$ The general relationship between the standard cell potential $E_{\text {cell }}^{\circ}$ and the equilibrium constant $K$ is given by the Nernst equation, specifically in its standard form: $E_{\mathrm{cell}}^{\circ}=\frac{0.0592}{n} \log _{10}(K)$

Asked in: MHT CET 2024 (16 May Shift 2)

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