Which Of The Following Is Not An Oxidation-reduction Reaction?A. X E F 6 ( S ) ⟶ X E F 4 ( S ) + F 2 ( G XeF_6(s) \longrightarrow XeF_4(s) + F_2(g X E F 6 ( S ) ⟶ X E F 4 ( S ) + F 2 ( G ]B. 2 C S ( S ) + I 2 ( G ) ⟶ 2 C S I ( S 2Cs(s) + I_2(g) \longrightarrow 2CsI(s 2 C S ( S ) + I 2 ( G ) ⟶ 2 C S I ( S ]C. $2H_2SO_4(aq) + 2Ba(OH)_2(aq) \longrightarrow 2BaSO_4(s) +

Mar 12, 2025 by ADMIN 377 views

Which of the Following is Not an Oxidation-Reduction Reaction?

Understanding Oxidation-Reduction Reactions

Oxidation-reduction reactions, also known as redox reactions, are a fundamental concept in chemistry. These reactions involve the transfer of electrons between two substances, resulting in a change in oxidation state. Oxidation is the loss of electrons, while reduction is the gain of electrons. Redox reactions are crucial in various chemical processes, including combustion, corrosion, and the synthesis of compounds.

Examples of Oxidation-Reduction Reactions

To understand which of the given reactions is not an oxidation-reduction reaction, let's first examine the examples provided:

A. $XeF_6(s) \longrightarrow XeF_4(s) + F_2(g)$

This reaction involves the decomposition of xenon hexafluoride (XeF6) into xenon tetrafluoride (XeF4) and fluorine gas (F2). In this reaction, the oxidation state of xenon changes from +6 to +4, while the oxidation state of fluorine remains the same. This reaction is an example of a redox reaction, as it involves the transfer of electrons.

B. $2Cs(s) + I_2(g) \longrightarrow 2CsI(s)$

This reaction involves the reaction of cesium metal (Cs) with iodine gas (I2) to form cesium iodide (CsI). In this reaction, the oxidation state of cesium changes from 0 to +1, while the oxidation state of iodine changes from 0 to -1. This reaction is an example of a redox reaction, as it involves the transfer of electrons.

C. $2H_2SO_4(aq) + 2Ba(OH)_2(aq) \longrightarrow 2BaSO_4(s) + 4H_2O(l)$

This reaction involves the reaction of sulfuric acid (H2SO4) with barium hydroxide (Ba(OH)2) to form barium sulfate (BaSO4) and water (H2O). In this reaction, the oxidation state of sulfur changes from +6 to +6, while the oxidation state of barium changes from +2 to +2. This reaction is an example of an acid-base reaction, not a redox reaction.

Analyzing the Reactions

Based on the analysis above, it is clear that reactions A and B are examples of oxidation-reduction reactions, as they involve the transfer of electrons and a change in oxidation state. On the other hand, reaction C is an example of an acid-base reaction, as it involves the transfer of hydrogen ions and a change in pH, but not a change in oxidation state.

Conclusion

In conclusion, the correct answer to the question is C. $2H_2SO_4(aq) + 2Ba(OH)_2(aq) \longrightarrow 2BaSO_4(s) + 4H_2O(l)$ . This reaction is not an oxidation-reduction reaction, as it does not involve the transfer of electrons and a change in oxidation state. Instead, it is an example of an acid-base reaction.

Key Takeaways

Oxidation-reduction reactions involve the transfer of electrons and a change in oxidation state.
Examples of oxidation-reduction reactions include combustion, corrosion, and the synthesis of compounds.
Acid-base reactions involve the transfer of hydrogen ions and a change in pH, but not a change in oxidation state.
Understanding the difference between oxidation-reduction reactions and acid-base reactions is crucial in chemistry.

Further Reading

For further reading on oxidation-reduction reactions and acid-base reactions, we recommend the following resources:

"Chemistry: The Central Science" by Theodore L. Brown, H. Eugene LeMay, and Bruce E. Bursten
"General Chemistry: Principles and Modern Applications" by Linus Pauling
"Chemistry: An Atoms First Approach" by Steven S. Zumdahl

References

Brown, T. L., LeMay, H. E., & Bursten, B. E. (2017). Chemistry: The Central Science. Pearson Education.
Pauling, L. (1988). General Chemistry: Principles and Modern Applications. Dover Publications.
Zumdahl, S. S. (2014). Chemistry: An Atoms First Approach. Cengage Learning.
Q&A: Oxidation-Reduction Reactions and Acid-Base Reactions

Understanding Oxidation-Reduction Reactions and Acid-Base Reactions

Oxidation-reduction reactions and acid-base reactions are two fundamental concepts in chemistry. While both types of reactions involve the transfer of electrons or ions, they differ in their mechanisms and outcomes. In this article, we will answer some frequently asked questions about oxidation-reduction reactions and acid-base reactions.

Q: What is an oxidation-reduction reaction?

A: An oxidation-reduction reaction, also known as a redox reaction, is a chemical reaction that involves the transfer of electrons between two substances, resulting in a change in oxidation state. Oxidation is the loss of electrons, while reduction is the gain of electrons.

Q: What is an acid-base reaction?

A: An acid-base reaction is a chemical reaction that involves the transfer of hydrogen ions (H+) and a change in pH. In an acid-base reaction, an acid donates a hydrogen ion, while a base accepts a hydrogen ion.

Q: What is the difference between an oxidation-reduction reaction and an acid-base reaction?

A: The main difference between an oxidation-reduction reaction and an acid-base reaction is the mechanism of the reaction. Oxidation-reduction reactions involve the transfer of electrons, while acid-base reactions involve the transfer of hydrogen ions.

Q: Can an acid-base reaction be an oxidation-reduction reaction?

A: Yes, some acid-base reactions can also be oxidation-reduction reactions. For example, the reaction between hydrogen peroxide (H2O2) and acid can be both an acid-base reaction and an oxidation-reduction reaction.

Q: What are some examples of oxidation-reduction reactions?

A: Some examples of oxidation-reduction reactions include:

Combustion reactions, such as the burning of gasoline or wood
Corrosion reactions, such as the rusting of iron
Synthesis reactions, such as the formation of water from hydrogen and oxygen

Q: What are some examples of acid-base reactions?

A: Some examples of acid-base reactions include:

The reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O)
The reaction between sulfuric acid (H2SO4) and calcium hydroxide (Ca(OH)2) to form calcium sulfate (CaSO4) and water (H2O)

Q: How can I determine if a reaction is an oxidation-reduction reaction or an acid-base reaction?

A: To determine if a reaction is an oxidation-reduction reaction or an acid-base reaction, you can follow these steps:

Look for the transfer of electrons: If the reaction involves the transfer of electrons, it is likely an oxidation-reduction reaction.
Look for the transfer of hydrogen ions: If the reaction involves the transfer of hydrogen ions, it is likely an acid-base reaction.
Check the change in oxidation state: If the oxidation state of an atom changes, it is likely an oxidation-reduction reaction.

Q: What are some common mistakes to avoid when working with oxidation-reduction reactions and acid-base reactions?

A: Some common mistakes to avoid when working with oxidation-reduction reactions and acid-base reactions include:

Confusing oxidation-reduction reactions with acid-base reactions
Failing to balance the equation
Not considering the change in oxidation state
Not considering the transfer of hydrogen ions