A) \[M\,+\,X\,\to {{M}^{+}}+{{X}^{-}}\] is the spontaneous reaction
B) \[{{M}^{+}}+{{X}^{-}}\to M+X\] is the spontaneous reaction
C) \[{{E}_{cell}}\]= 0.77 V
D) \[{{E}_{cell}}\]= ? 0.77 V
Correct Answer: B
Solution :
For the given cell \[M|{{M}^{+}}||{{X}^{-}}|X\], the cell reaction is derived as follows: RHS: reduction \[X+{{e}^{-}}\to {{X}^{-}}\] ?..(i) LHS: Oxidation \[M\to {{M}^{+}}+{{e}^{-}}\] ?..(ii) Add (i) and (ii) \[M+X\to {{M}^{+}}+{{X}^{-}}\] The cell potential = \[-0.11\,V\] Since \[{{E}_{cell}}=\]? ve, the cell reaction derived above is not spontaneous. In fact, the reverse reaction will occur spontaneously.
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