Consider The Redox Reaction Below:${ 2 \text{Al(s)} + 6 \text{HCl(aq)} \longrightarrow 2 \text{AlCl}_3\text{(aq)} + 3 \text{H}_2\text{(g)} }$Which Statement Correctly Describes A Half-reaction That Is Taking Place?A. Hydrogen Is Oxidized

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Redox reactions are a fundamental concept in chemistry, involving the transfer of electrons between two species. These reactions are crucial in understanding various chemical processes, including combustion, corrosion, and electrochemistry. In this article, we will delve into the given redox reaction and identify the half-reaction that is taking place.

The Given Redox Reaction

The given redox reaction is:

2Al(s)+6HCl(aq)⟶2AlCl3(aq)+3H2(g){ 2 \text{Al(s)} + 6 \text{HCl(aq)} \longrightarrow 2 \text{AlCl}_3\text{(aq)} + 3 \text{H}_2\text{(g)} }

This reaction involves the reaction of aluminum (Al) with hydrochloric acid (HCl) to produce aluminum chloride (AlCl3) and hydrogen gas (H2).

Identifying Half-Reactions

To identify the half-reaction that is taking place, we need to understand the concept of oxidation and reduction. Oxidation is the loss of electrons, while reduction is the gain of electrons. A half-reaction is a reaction that involves either oxidation or reduction.

Oxidation and Reduction in the Given Reaction

In the given reaction, aluminum (Al) is losing electrons to form aluminum chloride (AlCl3), while hydrogen (H) is gaining electrons to form hydrogen gas (H2). This indicates that aluminum is being oxidized, and hydrogen is being reduced.

Half-Reaction Involving Oxidation

The half-reaction involving oxidation is:

2Al(s)⟶2Al3+(aq)+6e−{ 2 \text{Al(s)} \longrightarrow 2 \text{Al}^{3+}\text{(aq)} + 6 \text{e}^{-} }

In this half-reaction, aluminum (Al) is losing electrons to form aluminum ions (Al3+).

Half-Reaction Involving Reduction

The half-reaction involving reduction is:

6H+(aq)+6e−⟶3H2(g){ 6 \text{H}^{+}\text{(aq)} + 6 \text{e}^{-} \longrightarrow 3 \text{H}_2\text{(g)} }

In this half-reaction, hydrogen ions (H+) are gaining electrons to form hydrogen gas (H2).

Conclusion

In conclusion, the half-reaction that is taking place in the given redox reaction is the reduction of hydrogen ions (H+) to form hydrogen gas (H2). This is evident from the fact that hydrogen is gaining electrons to form hydrogen gas.

Answer to the Question

The correct answer to the question is:

A. Hydrogen is oxidized

However, this is incorrect. Hydrogen is actually being reduced, not oxidized.

Final Thoughts

Redox reactions are a fundamental concept in chemistry, and understanding them is crucial in various fields, including chemistry, physics, and engineering. By identifying the half-reactions involved in a redox reaction, we can gain a deeper understanding of the underlying chemical processes.

Understanding Oxidation and Reduction

Oxidation and reduction are two fundamental concepts in chemistry that are essential in understanding redox reactions. Oxidation is the loss of electrons, while reduction is the gain of electrons.

Examples of Oxidation and Reduction

  • Oxidation: The loss of electrons by a species, resulting in an increase in oxidation state.
  • Reduction: The gain of electrons by a species, resulting in a decrease in oxidation state.

Half-Reactions

Half-reactions are reactions that involve either oxidation or reduction. They are essential in understanding redox reactions and can be used to identify the half-reactions involved in a redox reaction.

Examples of Half-Reactions

  • Oxidation half-reaction: The loss of electrons by a species, resulting in an increase in oxidation state.
  • Reduction half-reaction: The gain of electrons by a species, resulting in a decrease in oxidation state.

Redox Reactions

Redox reactions are reactions that involve the transfer of electrons between two species. They are essential in understanding various chemical processes, including combustion, corrosion, and electrochemistry.

Examples of Redox Reactions

  • Combustion reactions: Reactions that involve the reaction of a fuel with oxygen, resulting in the release of heat and light.
  • Corrosion reactions: Reactions that involve the reaction of a metal with its environment, resulting in the degradation of the metal.
  • Electrochemical reactions: Reactions that involve the transfer of electrons between two species, resulting in the formation of a chemical compound.

Conclusion

Q: What is a redox reaction?

A: A redox reaction is a chemical reaction that involves the transfer of electrons between two species. It is a fundamental concept in chemistry that is essential in understanding various chemical processes, including combustion, corrosion, and electrochemistry.

Q: What is oxidation?

A: Oxidation is the loss of electrons by a species, resulting in an increase in oxidation state. It is a key concept in understanding redox reactions and can be represented by the following equation:

Oxidation:  A⟶An++ne−{ \text{Oxidation:} \ \ \text{A} \longrightarrow \text{A}^{n+} + n\text{e}^{-} }

Q: What is reduction?

A: Reduction is the gain of electrons by a species, resulting in a decrease in oxidation state. It is a key concept in understanding redox reactions and can be represented by the following equation:

Reduction:  An++ne−⟶A{ \text{Reduction:} \ \ \text{A}^{n+} + n\text{e}^{-} \longrightarrow \text{A} }

Q: What is a half-reaction?

A: A half-reaction is a reaction that involves either oxidation or reduction. It is a key concept in understanding redox reactions and can be used to identify the half-reactions involved in a redox reaction.

Q: What is the difference between a redox reaction and a half-reaction?

A: A redox reaction is a chemical reaction that involves the transfer of electrons between two species, while a half-reaction is a reaction that involves either oxidation or reduction. A redox reaction typically involves two half-reactions, one involving oxidation and the other involving reduction.

Q: How do you identify the half-reactions involved in a redox reaction?

A: To identify the half-reactions involved in a redox reaction, you need to determine which species is being oxidized and which species is being reduced. This can be done by looking at the change in oxidation state of the species involved in the reaction.

Q: What is the role of electrons in a redox reaction?

A: Electrons play a crucial role in a redox reaction, as they are transferred from one species to another. The transfer of electrons is what drives the reaction and allows the species to change their oxidation state.

Q: Can you give an example of a redox reaction?

A: Yes, a classic example of a redox reaction is the reaction between zinc (Zn) and copper (Cu) ions:

Zn(s)+Cu2+(aq)⟶Zn2+(aq)+Cu(s){ \text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \longrightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)} }

In this reaction, zinc is being oxidized, while copper is being reduced.

Q: What is the significance of redox reactions in everyday life?

A: Redox reactions play a crucial role in various aspects of everyday life, including:

  • Combustion reactions: Redox reactions are involved in combustion reactions, such as the burning of fossil fuels.
  • Corrosion reactions: Redox reactions are involved in corrosion reactions, such as the rusting of iron.
  • Electrochemical reactions: Redox reactions are involved in electrochemical reactions, such as the charging of batteries.

Q: Can you summarize the key concepts of redox reactions?

A: Yes, the key concepts of redox reactions include:

  • Oxidation: The loss of electrons by a species, resulting in an increase in oxidation state.
  • Reduction: The gain of electrons by a species, resulting in a decrease in oxidation state.
  • Half-reactions: Reactions that involve either oxidation or reduction.
  • Redox reactions: Chemical reactions that involve the transfer of electrons between two species.

By understanding these key concepts, you can gain a deeper understanding of redox reactions and their significance in various aspects of everyday life.