Q95 / 200 · NEET 2011 (Screening) · Chemistry

If the $E_{\text {cell }}^{\circ}$ for a given reaction has a negative value then which of the following gives the correct relationships for the values of $\Delta G^{\circ}$ and $K_{\mathrm{eq}}$ ?

  • A
    $\Delta G^{\circ} < 0 ; K_{\mathrm{eq}}>1$
  • B
    $\Delta G^{\circ} < 0 ; K_{\text {eq }} < 1$
  • Correct answer
    C
    $\Delta G^{\circ}>0 ; K_{\mathrm{eq}} < 1$
  • D
    $\Delta G^{\circ}>0 ; K_{\text {eq }}>1$

Solution

$\Delta G^{\circ}=-n F E^{\circ}$ When $E^{\circ}$ is negative, then $\Delta G^{\circ}>0$ $\Delta G^{\circ}=-R T \ln K_{e q}$ When $\Delta G^{\circ}>0, K_{e q}=10^{-x}$ which is less than one, $i e, K_{e q} < 1$.

Hence, the correct answer is option: 'C'.

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