Answer
Yes, a spontaneous reaction will occur when a strip of Magnesium metal is dipped into a solution containing silver ions.
Half reactions:
Oxidation reaction: $Mg(s) -> Mg^{2+}(aq) + 2e^{-}$
Reduction reaction: $Ag^{+} (aq) + e^{-} -> Ag (s) $
Overall reaction: $Mg(s) + 2Ag^{+}(aq) -> Mg^{2+} (aq) + 2Ag(s)$
Work Step by Step
When Mg metal is dipped into a solution of silver ion, it oxidizes and form $Mg^{2+}$ ion. On the other hand, silver ion reduces to Silver metal.
This reaction occurs spontaneously because if we look at the metal activity series, it is seen that Mg is more active than Ag in the series. So, Mg undergoes oxidation and ion of Ag undergoes reduction. More active metal always undergoes oxidation.
oxidation reaction: $Mg(s) -> Mg^{2+}(aq) $
after balancing charge, oxidation reaction: $Mg(s) -> Mg^{2+}(aq) + 2e^{-}$
Reduction reaction: $Ag^{+} (aq) -> Ag (s) $
After balancing charge, reduction reaction: $Ag^{+} (aq) + e^{-} -> Ag (s) $
now, we have to multiply oxidation reaction with co-efficient 1 and reduction reaction with co-efficient 2 so that no. of electrons in both the half reactions will be equal.
After multiplying oxidation reaction: $Mg(s) -> Mg^{2+}(aq) + 2e^{-}$
After multiplying reduction reaction: $2Ag^{+} (aq) + 2e^{-} -> 2Ag (s) $
After that, we add both half reactions so that electrons from both equation are eliminated and we get the overall reaction:
$Mg(s) + 2Ag^{+}(aq) -> Mg^{2+} (aq) + 2Ag(s)$
