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^-`

Step-by-step 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^-`