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For the electrochemical cell,$M|M^+||X^-|X,E^{\large\circ}(M^+|M)=0.44V$ and $E^{\large\circ}(X|X^-)=0.33V$.From this data one can deduce that

$\begin{array}{1 1}M+X\rightarrow M^++X^-\text{ is the spontaneous reaction}\\M^++X^-\rightarrow M+X\text{ is the spontaneous reaction}\\E_{cell}=0.77V\\E_{cell}=-0.77V\end{array} $

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Answer : $M^++X^-\rightarrow M+X$ is the spontaneous reaction
For the given cell,the reaction is
$X+e^-\rightarrow X^-$
$M\rightarrow M^++e^-$
$X+M\rightarrow X^-+M^+$
The cell potential is $E=E^{\large\circ}(X|X^-)-E^{\large\circ}(M^+|M)$=0.33V-0.44V=-0.11V
Since the cell potential is negative,the cell reaction is not spontaneous.
answered Jul 22, 2014 by sreemathi.v

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