The statement of the redox reactions is spontaneous as "[tex]Zn + Ag^{+}[/tex]→ [tex]Zn^{2+} + Ag[/tex] ".
A redox reaction is the process in which electrons are exchanged between two reactants that are involved. The oxidation number of a molecule, atom, or ion varies as a result of gaining or losing an electron.
If the standard electrode potential for the redox reaction, [tex]E^{0}[/tex], is positive, the redox reaction is spontaneous. That means, the reaction will move forward if [tex]E^{0}[/tex] is positive. In this reaction, silver ion is the oxidizing agent that readily accepts the electron to attain (stable configuration) the metal state, while Zn is a reducing agent which loses electrons (i.e., oxidized) by causing a reduction. It proceeds with[tex]E^{0}[/tex] redox reaction as given, the reaction moves forward and is considered to be spontaneous.
Hence the correct answer is [tex]Zn + Ag^{+}[/tex] → [tex]Zn^{2+} + Ag[/tex].
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