Answered

IDNLearn.com: Your reliable source for finding precise answers. Discover in-depth answers from knowledgeable professionals, providing you with the information you need.

Consider the redox reaction below:
[tex]\[ Zn (s) + 2 HCl (aq) \longrightarrow ZnCl_2 (aq) + H_2 (g) \][/tex]

Which half-reaction correctly describes the oxidation that is taking place?

A. \( Zn^{2+} (s) + 2 e^{-} (aq) \longrightarrow Zn (s) \)
B. \( Zn (s) \longrightarrow Zn^{2+} (aq) + 2 e^{-} \)
C. \( 2 H^{+} + 2 e^{-} \longrightarrow H_2 \)
D. [tex]\( H_2 + 2 e^{-} \longrightarrow 2 H^{+} \)[/tex]

Sagot :

GinnyAnsweridn
To determine which half-reaction correctly describes the oxidation process for the given redox reaction:

[tex]\[ Zn (s) + 2 HCl (aq) \longrightarrow ZnCl_2 (aq) + H_2 (g) \][/tex]

First, we need to identify the species that are being oxidized and reduced.

Step-by-Step Solution:

1. Identify Oxidation and Reduction:
- In a redox reaction, oxidation is the process of losing electrons, while reduction is the process of gaining electrons.
- Here, zinc (\(Zn (s)\)) and hydrogen ions (\(H^+ (aq)\)) from hydrochloric acid (\(HCl (aq)\)) are involved.

2. Zn Oxidation:
- Zinc (\(Zn\)) starts in a solid metallic form and ends as zinc ions (\(Zn^{2+}\)) in solution.
- The transition from \(Zn (s)\) to \(Zn^{2+} (aq)\) involves the loss of electrons:
[tex]\[ Zn (s) \longrightarrow Zn^{2+} (aq) + 2e^{-} \][/tex]
- This half-reaction shows zinc (\(Zn\)) losing two electrons to form \(Zn^{2+}\), indicating oxidation.

3. Analyze the Options:
Let's review each provided half-reaction option to determine which correctly describes oxidation:

- Option 1: \(Zn^{2+} (s) + 2e^{-} (aq) \longrightarrow Zn (s)\)
- This represents zinc ions (\(Zn^{2+}\)) gaining electrons to form solid zinc (\(Zn\)), which is a reduction process, not oxidation.

- Option 2: \(Zn (s) \longrightarrow Zn^{2+} (aq) + 2e^{-}\)
- This shows solid zinc (\(Zn\)) losing electrons to form zinc ions (\(Zn^{2+}\)), correctly describing the oxidation process.

- Option 3: \(2 H^+ + 2e^{-} \longrightarrow H_2\)
- This represents hydrogen ions (\(H^+\)) gaining electrons to form hydrogen gas (\(H_2\)), which is a reduction process, not oxidation.

- Option 4: \(H_2 + 2e^{-} \longrightarrow 2 H^+\)
- This shows hydrogen gas (\(H_2\)) losing electrons to form hydrogen ions (\(H^+\)), which describes an oxidation process for hydrogen but not for zinc.

4. Conclusion:
- Based on the analysis, the correct half-reaction that describes the oxidation process for zinc (\(Zn\)) in the given redox reaction is:

[tex]\[ Zn (s) \longrightarrow Zn^{2+} (aq) + 2e^{-} \][/tex]

Thus, the correct option is Option 2.
We value your presence here. Keep sharing knowledge and helping others find the answers they need. This community is the perfect place to learn together. Discover insightful answers at IDNLearn.com. We appreciate your visit and look forward to assisting you again.