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  • Help me please, - Electrochemistry - NEET-2

If the E°cell 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 Keq?

  • Option 1)

    \Delta G^{\circ}>0 \: ; \: K_{eq}>1

  • Option 2)

    \Delta G^{\circ}<0 \: ; \: K_{eq}>1

  • Option 3)

    \Delta G^{\circ}<0 \: ; \: K_{eq}<1

  • Option 4)

    \Delta G^{\circ}>0 \: ; \: K_{eq}<1

 

Answers (1)

best_answer

 

Gibbs energy of the reaction -

\Delta_{r}G=-nFE_{cell}

- wherein

\Delta _{r}G = gibbs energy of the reaction

E_{cell}= emf of the cell

nF = amount of charge passed

 

 \Delta G^{\circ} = -nFE^{\circ}_{cell}

If E^{\circ}_{cell}=-Ve\: then\: \Delta G^{\circ} =+Ve, > 0

\Delta G^{\circ} =-nRT\: log\: K_{eq}

For +Ve \Delta G^{\circ}, log\: K_{eq} is -Ve

\therefore K_{eq} <1


Option 1)

\Delta G^{\circ}>0 \: ; \: K_{eq}>1

This is incorrect option

Option 2)

\Delta G^{\circ}<0 \: ; \: K_{eq}>1

This is incorrect option

Option 3)

\Delta G^{\circ}<0 \: ; \: K_{eq}<1

This is incorrect option

Option 4)

\Delta G^{\circ}>0 \: ; \: K_{eq}<1

This is correct option

Posted by

Aadil

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