Aluminum Reacts With Oxygen To Form Aluminum Oxide:${ 4 \text{Al}(s) + 3 \text{O}_2(g) \rightarrow 2 \text{Al}_2\text{O}_3(s) }$How Many Moles Of { \text{O}_2$}$ Are Required To Completely React With 3.76 Moles Of

Mar 8, 2025 by ADMIN 215 views

The Reaction Between Aluminum and Oxygen: A Study of Stoichiometry

Chemical reactions are a fundamental aspect of chemistry, and understanding the stoichiometry of these reactions is crucial in determining the amount of reactants required to produce a specific amount of product. In this article, we will explore the reaction between aluminum and oxygen to form aluminum oxide, and calculate the number of moles of oxygen required to completely react with a given amount of aluminum.

The reaction between aluminum and oxygen is a classic example of a redox reaction, where aluminum loses electrons to form a positive ion, and oxygen gains electrons to form a negative ion. The balanced chemical equation for this reaction is:

${ 4 \text{Al}(s) + 3 \text{O}_2(g) \rightarrow 2 \text{Al}_2\text{O}_3(s) }$

In this equation, 4 moles of aluminum react with 3 moles of oxygen to form 2 moles of aluminum oxide.

To calculate the number of moles of oxygen required to completely react with 3.76 moles of aluminum, we can use the mole ratio from the balanced chemical equation. According to the equation, 4 moles of aluminum react with 3 moles of oxygen. Therefore, the mole ratio of aluminum to oxygen is:

${ \frac{\text{Al}}{\text{O}_2} = \frac{4}{3} }$

We can use this mole ratio to calculate the number of moles of oxygen required to react with 3.76 moles of aluminum. Let's call the number of moles of oxygen required "x". We can set up the following proportion:

${ \frac{4}{3} = \frac{3.76}{x} }$

To solve for x, we can cross-multiply and divide:

${ 4x = 3.76 \times 3 }$ ${ 4x = 11.28 }$ ${ x = \frac{11.28}{4} }$ ${ x = 2.82 }$

Therefore, 2.82 moles of oxygen are required to completely react with 3.76 moles of aluminum.

In conclusion, the reaction between aluminum and oxygen is a classic example of a redox reaction, where aluminum loses electrons to form a positive ion, and oxygen gains electrons to form a negative ion. By using the mole ratio from the balanced chemical equation, we can calculate the number of moles of oxygen required to completely react with a given amount of aluminum. In this case, 2.82 moles of oxygen are required to react with 3.76 moles of aluminum.

Stoichiometry is the study of the quantitative relationships between reactants and products in chemical reactions. The mole ratio is a fundamental concept in stoichiometry, and it is used to calculate the amount of reactants required to produce a specific amount of product.

The mole ratio is calculated by dividing the number of moles of one reactant by the number of moles of another reactant. In the case of the reaction between aluminum and oxygen, the mole ratio is:

${ \frac{\text{Al}}{\text{O}_2} = \frac{4}{3} }$

This means that for every 4 moles of aluminum, 3 moles of oxygen are required to react.

To calculate the number of moles of oxygen required to react with 3.76 moles of aluminum, we can use the mole ratio. Let's call the number of moles of oxygen required "x". We can set up the following proportion:

${ \frac{4}{3} = \frac{3.76}{x} }$

To solve for x, we can cross-multiply and divide:

${ 4x = 3.76 \times 3 }$ ${ 4x = 11.28 }$ ${ x = \frac{11.28}{4} }$ ${ x = 2.82 }$

Therefore, 2.82 moles of oxygen are required to completely react with 3.76 moles of aluminum.

Stoichiometry is a fundamental concept in chemistry, and it is used to calculate the amount of reactants required to produce a specific amount of product. The mole ratio is a key concept in stoichiometry, and it is used to calculate the amount of reactants required to react.

In this article, we have seen how the mole ratio can be used to calculate the number of moles of oxygen required to react with a given amount of aluminum. This is just one example of how stoichiometry is used in chemistry, and there are many other applications of this concept.

Stoichiometry has many real-world applications, including:

Chemical manufacturing: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in chemical manufacturing.
Pharmaceuticals: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in pharmaceuticals.
Environmental science: Stoichiometry is used to calculate the amount of pollutants released into the environment.
Food science: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in food science.

In conclusion, stoichiometry is a fundamental concept in chemistry, and it has many real-world applications. The mole ratio is a key concept in stoichiometry, and it is used to calculate the amount of reactants required to produce a specific amount of product.
Q&A: The Reaction Between Aluminum and Oxygen

A: The balanced chemical equation for the reaction between aluminum and oxygen is:

${ 4 \text{Al}(s) + 3 \text{O}_2(g) \rightarrow 2 \text{Al}_2\text{O}_3(s) }$

A: To calculate the number of moles of oxygen required to react with 3.76 moles of aluminum, we can use the mole ratio from the balanced chemical equation. According to the equation, 4 moles of aluminum react with 3 moles of oxygen. Therefore, the mole ratio of aluminum to oxygen is:

${ \frac{\text{Al}}{\text{O}_2} = \frac{4}{3} }$

${ \frac{4}{3} = \frac{3.76}{x} }$

To solve for x, we can cross-multiply and divide:

${ 4x = 3.76 \times 3 }$ ${ 4x = 11.28 }$ ${ x = \frac{11.28}{4} }$ ${ x = 2.82 }$

Therefore, 2.82 moles of oxygen are required to completely react with 3.76 moles of aluminum.

A: The mole ratio of aluminum to oxygen in the reaction between aluminum and oxygen is:

${ \frac{\text{Al}}{\text{O}_2} = \frac{4}{3} }$

This means that for every 4 moles of aluminum, 3 moles of oxygen are required to react.

A: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in the reaction between aluminum and oxygen. The mole ratio is a key concept in stoichiometry, and it is used to calculate the amount of reactants required to react.

A: Stoichiometry has many real-world applications, including:

Chemical manufacturing: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in chemical manufacturing.
Pharmaceuticals: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in pharmaceuticals.
Environmental science: Stoichiometry is used to calculate the amount of pollutants released into the environment.
Food science: Stoichiometry is used to calculate the amount of reactants required to produce a specific amount of product in food science.

A: Understanding stoichiometry is important because it allows us to calculate the amount of reactants required to produce a specific amount of product. This is crucial in many fields, including chemical manufacturing, pharmaceuticals, environmental science, and food science.

A: You can apply stoichiometry to your own life by using it to calculate the amount of reactants required to produce a specific amount of product in various fields. For example, you can use stoichiometry to calculate the amount of ingredients required to make a specific recipe in food science.

A: Some common mistakes to avoid when using stoichiometry include:

Not balancing the chemical equation: Make sure to balance the chemical equation before using stoichiometry.
Not using the correct mole ratio: Make sure to use the correct mole ratio from the balanced chemical equation.
Not converting units correctly: Make sure to convert units correctly when using stoichiometry.

By understanding stoichiometry and avoiding common mistakes, you can apply it to your own life and make informed decisions in various fields.