Consider The Chemical Reaction Below.${ Zn(s) + 2H^{+}(aq) \longrightarrow Zn^{2+}(aq) + H_2(g) }$Which Half-reaction Correctly Represents Reduction For This Equation?A. { Zn \longrightarrow Zn^{2+}(aq) + 2e^{-} $} B . \[ B. \[ B . \[

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Introduction

Redox reactions are a fundamental concept in chemistry, involving the transfer of electrons between species. These reactions are crucial in understanding various chemical processes, including combustion, corrosion, and electrochemistry. In this article, we will delve into the world of redox reactions, focusing on identifying the correct half-reaction for a given equation.

What are Redox Reactions?

Redox reactions involve the transfer of electrons from one species to another. The term "redox" is a combination of the words "reduction" and "oxidation." Reduction is the gain of electrons, while oxidation is the loss of electrons. In a redox reaction, one species is reduced, while another is oxidized.

The Given Chemical Reaction

The chemical reaction provided is:

Zn(s)+2H+(aq)⟶Zn2+(aq)+H2(g){ Zn(s) + 2H^{+}(aq) \longrightarrow Zn^{2+}(aq) + H_2(g) }

In this reaction, zinc (Zn) is in its solid state, and hydrogen ions (H+) are in aqueous solution. The products are zinc ions (Zn2+) in aqueous solution and hydrogen gas (H2).

Identifying the Correct Half-Reaction

To identify the correct half-reaction, we need to determine which species is being reduced and which is being oxidized. In the given reaction, zinc (Zn) is being oxidized, as it loses electrons to form zinc ions (Zn2+). On the other hand, hydrogen ions (H+) are being reduced, as they gain electrons to form hydrogen gas (H2).

Option A: Incorrect Half-Reaction

Option A is:

Zn⟶Zn2+(aq)+2e−{ Zn \longrightarrow Zn^{2+}(aq) + 2e^{-} }

This half-reaction represents the oxidation of zinc, but it is incomplete. The correct representation of the oxidation of zinc should include the loss of electrons, which is not shown in this option.

Option B: Correct Half-Reaction

Option B is:

2H+(aq)+2e−⟶H2(g){ 2H^{+}(aq) + 2e^{-} \longrightarrow H_2(g) }

This half-reaction represents the reduction of hydrogen ions, as they gain electrons to form hydrogen gas. This is the correct representation of the reduction half-reaction for the given equation.

Conclusion

In conclusion, the correct half-reaction for the given equation is the reduction of hydrogen ions, as represented by Option B. This half-reaction accurately shows the gain of electrons by hydrogen ions to form hydrogen gas. Understanding redox reactions and identifying the correct half-reaction is crucial in various fields of chemistry, including electrochemistry and corrosion science.

Key Takeaways

  • Redox reactions involve the transfer of electrons between species.
  • Reduction is the gain of electrons, while oxidation is the loss of electrons.
  • The given chemical reaction involves the oxidation of zinc and the reduction of hydrogen ions.
  • The correct half-reaction for the given equation is the reduction of hydrogen ions, as represented by Option B.

Further Reading

For further reading on redox reactions and half-reactions, we recommend the following resources:

  • "Redox Reactions" by the Royal Society of Chemistry
  • "Half-Reactions" by the American Chemical Society
  • "Redox Chemistry" by the National Institute of Standards and Technology

Introduction

Redox reactions are a fundamental concept in chemistry, involving the transfer of electrons between species. In our previous article, we discussed the basics of redox reactions and identified the correct half-reaction for a given equation. In this article, we will continue to explore redox reactions through a Q&A format, providing answers to common questions and clarifying any misconceptions.

Q1: What is the difference between oxidation and reduction?

A1: Oxidation is the loss of electrons, while reduction is the gain of electrons. In a redox reaction, one species is oxidized, while another is reduced.

Q2: How do I identify the oxidized and reduced species in a redox reaction?

A2: To identify the oxidized and reduced species, look for the species that loses electrons (oxidized) and the species that gains electrons (reduced). You can also use the following rules:

  • If a species loses oxygen or gains hydrogen, it is oxidized.
  • If a species gains oxygen or loses hydrogen, it is reduced.

Q3: What is the role of electrons in a redox reaction?

A3: 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, allowing the species to change their oxidation state.

Q4: How do I balance a redox reaction?

A4: Balancing a redox reaction involves ensuring that the number of electrons lost by the oxidized species is equal to the number of electrons gained by the reduced species. You can use the following steps:

  1. Write the unbalanced equation.
  2. Separate the equation into two half-reactions: oxidation and reduction.
  3. Balance each half-reaction separately.
  4. Combine the two balanced half-reactions to form the overall balanced equation.

Q5: What is the difference between a redox reaction and a chemical reaction?

A5: A redox reaction is a type of chemical reaction that involves the transfer of electrons between species. While all redox reactions are chemical reactions, not all chemical reactions are redox reactions.

Q6: Can a redox reaction occur in a single step?

A6: Yes, a redox reaction can occur in a single step. However, it is more common for redox reactions to occur in multiple steps, with the transfer of electrons occurring over a series of intermediate species.

Q7: How do I determine the standard reduction potential (E°) of a species?

A7: The standard reduction potential (E°) of a species is a measure of its tendency to gain electrons. You can determine the E° of a species by measuring the potential difference between the species and a standard electrode (such as the standard hydrogen electrode).

Q8: What is the significance of the standard reduction potential (E°) in redox reactions?

A8: The standard reduction potential (E°) is a crucial parameter in redox reactions, as it determines the direction of the reaction. A species with a more negative E° will be reduced, while a species with a more positive E° will be oxidized.

Conclusion

In conclusion, redox reactions are a fundamental concept in chemistry, involving the transfer of electrons between species. By understanding the basics of redox reactions and identifying the correct half-reaction, you will be better equipped to tackle complex chemical problems and make informed decisions in various fields of chemistry. We hope this Q&A article has provided you with a deeper understanding of redox reactions and has answered any questions you may have had.

Key Takeaways

  • Redox reactions involve the transfer of electrons between species.
  • Oxidation is the loss of electrons, while reduction is the gain of electrons.
  • The standard reduction potential (E°) is a measure of a species' tendency to gain electrons.
  • Redox reactions can occur in a single step or multiple steps.

Further Reading

For further reading on redox reactions and half-reactions, we recommend the following resources:

  • "Redox Reactions" by the Royal Society of Chemistry
  • "Half-Reactions" by the American Chemical Society
  • "Redox Chemistry" by the National Institute of Standards and Technology

By continuing to explore redox reactions, you will gain a deeper understanding of this fundamental concept in chemistry and be better equipped to tackle complex chemical problems.