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Question
Answer the following:
Predict whether the following reaction would occur spontaneously under standard state condition.
\[\ce{2Ag_{(s)} + Ni^{2+}_{ (aq)} -> 2Ag^{+}_{ (aq)} + Ni_{(s)}}\]
Solution
\[\ce{2Ag_{(s)} + Ni^{2+}_{ (aq)} -> 2Ag^{+}_{ (aq)} + Ni_{(s)}}\]
At anode: \[\ce{2Ag_{(s)} -> 2Ag^+_{ (aq)} + 2e^-}\]
At cathode: \[\ce{Ni^{2+}_{ (aq)} + 2e^- -> Ni_{(s)}}\]
From the electrochemical series we have,
`"E"_("Ag")^circ` = 0.799 V and `"E"_"Ni"^circ` = - 0.257 V
For cell having Ag as anode and Ni as cathode.
`"E"_"cell"^circ = "E"_"Ni"^circ - "E"_"Ag"^circ`
= - 0.257 V - 0.799 V
`"E"_"cell"^circ` = - 1.056 V
Emf of cell being negative, the given cell reaction is nonspontaneous.
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