Consider The Reaction Below:${ 2 \text{Al}_2 \text{O}_3 \rightarrow 4 \text{Al} + 3 \text{O}_2 }$How Many Moles Of Oxygen Are Produced When 26.5 Mol Of Aluminum Oxide Are Decomposed?A. 17.7 Mol B. 19.9 Mol C. 39.8 Mol D. 53.0 Mol

Introduction

In chemistry, decomposition reactions involve the breakdown of a compound into simpler substances. The reaction of aluminum oxide (Al2O3) is a classic example of a decomposition reaction, where aluminum oxide decomposes into aluminum (Al) and oxygen (O2). In this article, we will explore the decomposition reaction of aluminum oxide and calculate the number of moles of oxygen produced when a given amount of aluminum oxide is decomposed.

The Decomposition Reaction

The decomposition reaction of aluminum oxide is represented by the following equation:

${ 2 \text{Al}_2 \text{O}_3 \rightarrow 4 \text{Al} + 3 \text{O}_2 }$

In this reaction, 2 moles of aluminum oxide (Al2O3) decompose into 4 moles of aluminum (Al) and 3 moles of oxygen (O2). This reaction is a classic example of a decomposition reaction, where a single compound breaks down into multiple products.

Calculating the Number of Moles of Oxygen Produced

To calculate the number of moles of oxygen produced when a given amount of aluminum oxide is decomposed, we need to use the mole ratio between aluminum oxide and oxygen in the reaction equation. From the reaction equation, we can see that 2 moles of aluminum oxide produce 3 moles of oxygen. Therefore, the mole ratio between aluminum oxide and oxygen is 2:3.

Let's assume that we have 26.5 mol of aluminum oxide that is decomposed. To calculate the number of moles of oxygen produced, we can use the mole ratio between aluminum oxide and oxygen:

${ \text{moles of oxygen} = \frac{3}{2} \times \text{moles of aluminum oxide} }$

Substituting the given value of 26.5 mol of aluminum oxide, we get:

${ \text{moles of oxygen} = \frac{3}{2} \times 26.5 }$

${ \text{moles of oxygen} = 39.75 }$

Rounding off to one decimal place, we get:

${ \text{moles of oxygen} = 39.8 }$

Therefore, when 26.5 mol of aluminum oxide is decomposed, 39.8 mol of oxygen is produced.

Conclusion

In conclusion, the decomposition reaction of aluminum oxide is a classic example of a decomposition reaction, where a single compound breaks down into multiple products. By using the mole ratio between aluminum oxide and oxygen in the reaction equation, we can calculate the number of moles of oxygen produced when a given amount of aluminum oxide is decomposed. In this article, we calculated that when 26.5 mol of aluminum oxide is decomposed, 39.8 mol of oxygen is produced.

Answer

Q: What is the decomposition reaction of aluminum oxide?

A: The decomposition reaction of aluminum oxide is a chemical reaction where aluminum oxide (Al2O3) breaks down into aluminum (Al) and oxygen (O2). The reaction is represented by the following equation:

${ 2 \text{Al}_2 \text{O}_3 \rightarrow 4 \text{Al} + 3 \text{O}_2 }$

Q: What is the mole ratio between aluminum oxide and oxygen in the decomposition reaction?

A: The mole ratio between aluminum oxide and oxygen in the decomposition reaction is 2:3. This means that 2 moles of aluminum oxide produce 3 moles of oxygen.

Q: How many moles of oxygen are produced when 26.5 mol of aluminum oxide is decomposed?

A: To calculate the number of moles of oxygen produced, we can use the mole ratio between aluminum oxide and oxygen. The calculation is as follows:

${ \text{moles of oxygen} = \frac{3}{2} \times \text{moles of aluminum oxide} }$

Substituting the given value of 26.5 mol of aluminum oxide, we get:

${ \text{moles of oxygen} = \frac{3}{2} \times 26.5 }$

${ \text{moles of oxygen} = 39.75 }$

Rounding off to one decimal place, we get:

${ \text{moles of oxygen} = 39.8 }$

Therefore, when 26.5 mol of aluminum oxide is decomposed, 39.8 mol of oxygen is produced.

Q: What is the significance of the decomposition reaction of aluminum oxide?

A: The decomposition reaction of aluminum oxide is significant because it is a classic example of a decomposition reaction, where a single compound breaks down into multiple products. This reaction is also important in the production of aluminum metal, which is a widely used material in various industries.

Q: Can the decomposition reaction of aluminum oxide be reversed?

A: No, the decomposition reaction of aluminum oxide cannot be reversed. Once aluminum oxide is decomposed into aluminum and oxygen, it cannot be converted back into aluminum oxide.

Q: What are the products of the decomposition reaction of aluminum oxide?

A: The products of the decomposition reaction of aluminum oxide are aluminum (Al) and oxygen (O2).

Q: What is the balanced chemical equation for the decomposition reaction of aluminum oxide?

A: The balanced chemical equation for the decomposition reaction of aluminum oxide is:

${ 2 \text{Al}_2 \text{O}_3 \rightarrow 4 \text{Al} + 3 \text{O}_2 }$

Q: What is the role of heat in the decomposition reaction of aluminum oxide?

A: Heat is not a reactant in the decomposition reaction of aluminum oxide, but it is a necessary condition for the reaction to occur. The reaction requires a certain amount of heat energy to break the bonds between the aluminum and oxygen atoms in the aluminum oxide molecule.

Q: Can the decomposition reaction of aluminum oxide be used to produce oxygen gas?

A: Yes, the decomposition reaction of aluminum oxide can be used to produce oxygen gas. The reaction produces 3 moles of oxygen gas for every 2 moles of aluminum oxide decomposed.