Which Of The Reactions Is A Decomposition Reaction?A. 2 C 2 H 6 ( G ) + 7 O 2 ( G ) ⟶ 6 H 2 O ( L ) + 4 CO 2 ( G 2 \, \text{C}_2\text{H}_6(g) + 7 \, \text{O}_2(g) \longrightarrow 6 \, \text{H}_2\text{O}(l) + 4 \, \text{CO}_2(g 2 C 2 ​ H 6 ​ ( G ) + 7 O 2 ​ ( G ) ⟶ 6 H 2 ​ O ( L ) + 4 CO 2 ​ ( G ]B. $2 , \text{Al}(s) + 4 , \text{Cl}_2(g) \longrightarrow 2 ,

Introduction

Chemical reactions are an essential part of chemistry, and understanding the different types of reactions is crucial for any chemistry enthusiast. One of the fundamental types of reactions is decomposition reactions. In this article, we will explore what decomposition reactions are, how they differ from other types of reactions, and identify which of the given reactions is a decomposition reaction.

What is a Decomposition Reaction?

A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler substances. This type of reaction involves the breakdown of a compound into its constituent elements or simpler compounds. Decomposition reactions can be either spontaneous or induced by external factors such as heat, light, or pressure.

Characteristics of Decomposition Reactions

Decomposition reactions have several key characteristics that distinguish them from other types of reactions. Some of the key characteristics of decomposition reactions include:

• Single reactant: Decomposition reactions typically involve a single reactant that breaks down into two or more products.
• Breakdown of a compound: The reactant in a decomposition reaction is a compound that breaks down into simpler substances.
• No external reactant: Decomposition reactions do not require an external reactant to occur.
• Spontaneous or induced: Decomposition reactions can be either spontaneous or induced by external factors.

Examples of Decomposition Reactions

Some common examples of decomposition reactions include:

• Copper oxide decomposition: 2CuO(s) → 2Cu(s) + O2(g)
• Ammonium chloride decomposition: NH4Cl(s) → NH3(g) + HCl(g)
• Silver nitrate decomposition: 2AgNO3(s) → 2Ag(s) + 2NO2(g) + O2(g)

Analyzing the Given Reactions

Now that we have a good understanding of decomposition reactions, let's analyze the given reactions to determine which one is a decomposition reaction.

Reaction A

$2 \, \text{C}_2\text{H}_6(g) + 7 \, \text{O}_2(g) \longrightarrow 6 \, \text{H}_2\text{O}(l) + 4 \, \text{CO}_2(g)$

In this reaction, two molecules of ethane (C2H6) react with seven molecules of oxygen (O2) to produce six molecules of water (H2O) and four molecules of carbon dioxide (CO2). This reaction involves the breakdown of ethane into simpler substances, which is a characteristic of decomposition reactions.

Reaction B

$2 \, \text{Al}(s) + 4 \, \text{Cl}_2(g) \longrightarrow 2 \, \text{AlCl}_3(s)$

In this reaction, two atoms of aluminum (Al) react with four molecules of chlorine (Cl2) to produce two molecules of aluminum chloride (AlCl3). This reaction involves the combination of two elements to form a compound, which is not a characteristic of decomposition reactions.

Conclusion

Based on our analysis, Reaction A is a decomposition reaction because it involves the breakdown of a single compound (ethane) into simpler substances (water and carbon dioxide). Reaction B, on the other hand, is not a decomposition reaction because it involves the combination of two elements to form a compound.

Key Takeaways

• Decomposition reactions involve the breakdown of a single compound into two or more simpler substances.
• Characteristics of decomposition reactions include a single reactant, breakdown of a compound, no external reactant, and spontaneous or induced.
• Examples of decomposition reactions include copper oxide decomposition, ammonium chloride decomposition, and silver nitrate decomposition.
• Reaction A is a decomposition reaction, while Reaction B is not.

Frequently Asked Questions

• What is a decomposition reaction? A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler substances.
• What are the characteristics of decomposition reactions? The characteristics of decomposition reactions include a single reactant, breakdown of a compound, no external reactant, and spontaneous or induced.
• What are some examples of decomposition reactions? Examples of decomposition reactions include copper oxide decomposition, ammonium chloride decomposition, and silver nitrate decomposition.
• Which of the given reactions is a decomposition reaction? Reaction A is a decomposition reaction.
  Decomposition Reactions Q&A: Frequently Asked Questions ===========================================================

Introduction

In our previous article, we explored the basics of decomposition reactions, including their characteristics, examples, and how to identify them. In this article, we will answer some frequently asked questions about decomposition reactions to help you better understand this type of chemical reaction.

Q&A

Q: What is a decomposition reaction?

A: A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler substances.

Q: What are the characteristics of decomposition reactions?

A: The characteristics of decomposition reactions include:

• Single reactant: Decomposition reactions typically involve a single reactant that breaks down into two or more products.
• Breakdown of a compound: The reactant in a decomposition reaction is a compound that breaks down into simpler substances.
• No external reactant: Decomposition reactions do not require an external reactant to occur.
• Spontaneous or induced: Decomposition reactions can be either spontaneous or induced by external factors.

Q: What are some examples of decomposition reactions?

A: Some common examples of decomposition reactions include:

• Copper oxide decomposition: 2CuO(s) → 2Cu(s) + O2(g)
• Ammonium chloride decomposition: NH4Cl(s) → NH3(g) + HCl(g)
• Silver nitrate decomposition: 2AgNO3(s) → 2Ag(s) + 2NO2(g) + O2(g)

Q: How do I identify a decomposition reaction?

A: To identify a decomposition reaction, look for the following characteristics:

• Single reactant: Check if the reaction involves a single reactant that breaks down into two or more products.
• Breakdown of a compound: Check if the reactant is a compound that breaks down into simpler substances.
• No external reactant: Check if the reaction does not require an external reactant to occur.
• Spontaneous or induced: Check if the reaction is either spontaneous or induced by external factors.

Q: What are some common mistakes to avoid when identifying decomposition reactions?

A: Some common mistakes to avoid when identifying decomposition reactions include:

• Confusing decomposition reactions with combination reactions: Make sure to distinguish between decomposition reactions and combination reactions.
• Not considering the reactant: Make sure to consider the reactant in the reaction and check if it is a compound that breaks down into simpler substances.
• Not checking for external reactants: Make sure to check if the reaction requires an external reactant to occur.

Q: Can decomposition reactions be spontaneous or induced?

A: Yes, decomposition reactions can be either spontaneous or induced by external factors. Spontaneous decomposition reactions occur without any external influence, while induced decomposition reactions occur in response to external factors such as heat, light, or pressure.

Q: What are some real-world applications of decomposition reactions?

A: Decomposition reactions have several real-world applications, including:

• Production of chemicals: Decomposition reactions are used to produce various chemicals, such as ammonia and chlorine.
• Removal of pollutants: Decomposition reactions can be used to remove pollutants from the environment.
• Production of fuels: Decomposition reactions can be used to produce fuels, such as hydrogen and methane.

Conclusion

Decomposition reactions are an essential part of chemistry, and understanding them is crucial for any chemistry enthusiast. By answering some frequently asked questions about decomposition reactions, we hope to have provided you with a better understanding of this type of chemical reaction. Remember to always consider the characteristics of decomposition reactions, including single reactant, breakdown of a compound, no external reactant, and spontaneous or induced.

Key Takeaways

• Decomposition reactions involve the breakdown of a single compound into two or more simpler substances.
• Characteristics of decomposition reactions include single reactant, breakdown of a compound, no external reactant, and spontaneous or induced.
• Examples of decomposition reactions include copper oxide decomposition, ammonium chloride decomposition, and silver nitrate decomposition.
• Decomposition reactions can be spontaneous or induced by external factors.
• Real-world applications of decomposition reactions include production of chemicals, removal of pollutants, and production of fuels.

Frequently Asked Questions

• What is a decomposition reaction? A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler substances.
• What are the characteristics of decomposition reactions? The characteristics of decomposition reactions include single reactant, breakdown of a compound, no external reactant, and spontaneous or induced.
• What are some examples of decomposition reactions? Examples of decomposition reactions include copper oxide decomposition, ammonium chloride decomposition, and silver nitrate decomposition.
• How do I identify a decomposition reaction? To identify a decomposition reaction, look for the characteristics of decomposition reactions, including single reactant, breakdown of a compound, no external reactant, and spontaneous or induced.