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?\nzn²⁺(s) + 2e⁻(aq)→zn(s)\nzn(s)→zn²⁺(aq)+2e⁻\n2h⁺ + 2e⁻→h₂\nh₂ + 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?\nzn²⁺(s) + 2e⁻(aq)→zn(s)\nzn(s)→zn²⁺(aq)+2e⁻\n2h⁺ + 2e⁻→h₂\nh₂ + 2e⁻→2h⁺

Answer

Answer:

Zn(s) → Zn²⁺(aq) + 2e⁻

Explanation:

Step1: Define oxidation

Oxidation is loss of electrons.

Step2: Analyze Zn in reaction

In Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g), Zn goes from 0 oxidation - state in Zn(s) to + 2 oxidation - state in ZnCl₂.

Step3: Write oxidation half - reaction

Zn loses 2 electrons to form Zn²⁺, so the oxidation half - reaction is Zn(s) → Zn²⁺(aq) + 2e⁻.