Answer: The oxidation half reaction for the given reaction is [tex]Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-[/tex]
Explanation:
Oxidation reaction is defined as the reaction in which a substance looses its electron. The oxidation state of the substance gets increased.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.
[tex]X^{n+}+ne^-\rightarrow X[/tex]
For the given chemical equation:
[tex]Zn(s)+2HCl(aq.)\rightarrow ZnCl_2(aq.)+H_2(g)[/tex]
Oxidation half reaction: [tex]Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-[/tex]
Reduction half reaction: [tex]2H^+(aq.)+2e^-\rightarrow H_2(g)[/tex]
Zinc is getting oxidized and hydrogen is getting reduced.
Hence, the oxidation half reaction for the given reaction is [tex]Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-[/tex]
