Answer:
Overall balanced redox reaction :
[tex]Ni^{2+} (aq)+Zn(s)\rightarrow Ni(s)+Zn^{2+} (aq)[/tex]
Explanation:
[tex]Ni^{2+} (aq) +2e^-\rightarrow Ni(s)[/tex]..(1)
[tex]Zn(s)\rightarrow Zn^{2+} (aq) +2e^-[/tex] ..(2)
Oxidation reaction is a chemical reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reaction number 2 is an oxidation half reaction, in which zinc is loosing 2 electrons and forms zinc ion with +2 charge.
Reduction reaction is a chemical reaction in which an atom gains electrons. Here, the oxidation state of the atom decreases.
[tex]X^{n+}+ne^-\rightarrow X[/tex]
Reaction number 1 is a reduction half reaction, in which nickel ion with 2+ charge is gaining 2 electrons and forms nickel atoms.
Overall balanced redox reaction can be written adding (1) and (2):
[tex]Ni^{2+}+ (aq) 2e^-+Zn(s)\rightarrow Ni(s)+Zn^{2+} (aq) +2e^-[/tex]
[tex]Ni^{2+} (aq)+Zn(s)\rightarrow Ni(s)+Zn^{2+} (aq)[/tex]
