consider the redox reaction below.\nzn(s) + 2hcl(aq)→zncl2(aq) + h2(g)\nwhich half - reaction correctly…

consider the redox reaction below.\nzn(s) + 2hcl(aq)→zncl2(aq) + h2(g)\nwhich half - reaction correctly describes the oxidation that is taking place?\no zn2+(s) + 2e−(aq)→zn(s)\no zn(s)→zn2+(aq)+2e−\no 2h+ + 2e−→h2\no h2 + 2e−→2h+

consider the redox reaction below.\nzn(s) + 2hcl(aq)→zncl2(aq) + h2(g)\nwhich half - reaction correctly describes the oxidation that is taking place?\no zn2+(s) + 2e−(aq)→zn(s)\no zn(s)→zn2+(aq)+2e−\no 2h+ + 2e−→h2\no h2 + 2e−→2h+

Answer

Explanation:

Step1: Define oxidation

Oxidation is the loss of electrons.

Step2: Analyze Zn in the reaction

In the reaction $Zn(s)+2HCl(aq)\longrightarrow ZnCl_2(aq) + H_2(g)$, zinc starts as elemental zinc ($Zn(s)$) with an oxidation - state of 0 and ends up as $Zn^{2 + }$ in $ZnCl_2$ with an oxidation - state of + 2. Zinc loses 2 electrons.

Step3: Identify the oxidation half - reaction

The half - reaction that shows zinc losing 2 electrons is $Zn(s)\longrightarrow Zn^{2+}(aq)+2e^-$.

Answer:

$Zn(s)\longrightarrow Zn^{2+}(aq)+2e^-$