Question

Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) Which half reaction correctly describes the oxidation that is taking place?

Answer 1

Zn (s) -> Zn+2 (aq) + 2e-

Zn (s) with a neutral charge is oxidized and looses two electrons in the process to form ZnCl2 (aq) where Zn has a charge of 2+.

Answer 2

Answer: The oxidation half reaction for the given reaction is $Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-$

Explanation:

Oxidation reaction is defined as the reaction in which a substance looses its electron. The oxidation state of the substance gets increased.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

$X^{n+}+ne^-\rightarrow X$

For the given chemical equation:

$Zn(s)+2HCl(aq.)\rightarrow ZnCl_2(aq.)+H_2(g)$

Oxidation half reaction: $Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-$

Reduction half reaction: $2H^+(aq.)+2e^-\rightarrow H_2(g)$

Zinc is getting oxidized and hydrogen is getting reduced.

Hence, the oxidation half reaction for the given reaction is $Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-$