Given The Chemical Reaction: 2 Al + 6 HCl → 2 AlCl 3 + 3 H 2 2 \text{Al} + 6 \text{HCl} \rightarrow 2 \text{AlCl}_3 + 3 \text{H}_2 2 Al + 6 HCl → 2 AlCl 3 ​ + 3 H 2 ​ If The Chemical Reaction Produces 129 Grams Of AlCl 3 \text{AlCl}_3 AlCl 3 ​ , How Many Grams Of H 2 \text{H}_2 H 2 ​ Are Also Produced?A. 1.22 B.

Introduction

Chemical reactions are the foundation of chemistry, and understanding the relationships between reactants and products is crucial for predicting the outcomes of these reactions. One of the most important concepts in chemistry is stoichiometry, which deals with the quantitative relationships between reactants and products in chemical reactions. In this article, we will explore the concept of stoichiometry and how it can be applied to balance chemical equations and predict the amounts of products formed.

What is Stoichiometry?

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the calculation of the amounts of reactants and products required to produce a specific amount of a product. Stoichiometry is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

Balancing Chemical Equations

Balancing chemical equations is a crucial step in stoichiometry. A balanced chemical equation is one in which the number of atoms of each element is the same on both the reactant and product sides. This is achieved by adding coefficients in front of the formulas of the reactants and products. The coefficients are used to indicate the number of molecules of each reactant and product that participate in the reaction.

The Given Chemical Reaction

The given chemical reaction is:

$$2 \text{Al} + 6 \text{HCl} \rightarrow 2 \text{AlCl}_3 + 3 \text{H}_2$$

This reaction involves the reaction of aluminum (Al) with hydrochloric acid (HCl) to produce aluminum chloride (AlCl3) and hydrogen gas (H2).

Calculating the Amount of H2 Produced

To calculate the amount of H2 produced, we need to use the concept of stoichiometry. We are given that the reaction produces 129 grams of AlCl3. We need to find the amount of H2 produced.

First, we need to calculate the number of moles of AlCl3 produced. The molar mass of AlCl3 is 133.34 g/mol. We can calculate the number of moles of AlCl3 produced as follows:

$$\text{Number of moles of AlCl}_3 = \frac{\text{Mass of AlCl}_3}{\text{Molar mass of AlCl}_3}$$

$$\text{Number of moles of AlCl}_3 = \frac{129 \text{ g}}{133.34 \text{ g/mol}}$$

$$\text{Number of moles of AlCl}_3 = 0.975 \text{ mol}$$

Next, we need to use the mole ratio between AlCl3 and H2 to calculate the number of moles of H2 produced. From the balanced equation, we can see that 2 moles of AlCl3 are produced for every 3 moles of H2. Therefore, the mole ratio between AlCl3 and H2 is 2:3.

We can calculate the number of moles of H2 produced as follows:

$$\text{Number of moles of H}_2 = \frac{\text{Number of moles of AlCl}_3 \times 3}{2}$$

$$\text{Number of moles of H}_2 = \frac{0.975 \text{ mol} \times 3}{2}$$

$$\text{Number of moles of H}_2 = 1.4625 \text{ mol}$$

Finally, we can calculate the mass of H2 produced by multiplying the number of moles of H2 by its molar mass (2.016 g/mol).

$$\text{Mass of H}_2 = \text{Number of moles of H}_2 \times \text{Molar mass of H}_2$$

$$\text{Mass of H}_2 = 1.4625 \text{ mol} \times 2.016 \text{ g/mol}$$

$$\text{Mass of H}_2 = 2.95 \text{ g}$$

Therefore, the amount of H2 produced is 2.95 grams.

Conclusion

In this article, we have explored the concept of stoichiometry and how it can be applied to balance chemical equations and predict the amounts of products formed. We have used the given chemical reaction to calculate the amount of H2 produced when 129 grams of AlCl3 are produced. The calculation involves the use of mole ratios and molar masses to determine the number of moles of H2 produced and then the mass of H2 produced.

References

• Chemistry: An Atoms First Approach by Steven S. Zumdahl
• General Chemistry: Principles and Modern Applications by Linus Pauling
• Chemical Equations and Stoichiometry by the American Chemical Society

Further Reading

• Balancing Chemical Equations by the American Chemical Society
• Stoichiometry by the Khan Academy
• Chemical Reactions and Stoichiometry by the University of California, Berkeley

FAQs

• Q: What is stoichiometry? A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.
• Q: How do I balance a chemical equation? A: To balance a chemical equation, you need to add coefficients in front of the formulas of the reactants and products to ensure that the number of atoms of each element is the same on both the reactant and product sides.
• Q: How do I calculate the amount of a product formed in a chemical reaction? A: To calculate the amount of a product formed in a chemical reaction, you need to use the concept of stoichiometry and the mole ratio between the reactants and products.
  Frequently Asked Questions (FAQs) on Stoichiometry and Chemical Reactions ====================================================================

Q: What is stoichiometry?

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the calculation of the amounts of reactants and products required to produce a specific amount of a product.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to add coefficients in front of the formulas of the reactants and products to ensure that the number of atoms of each element is the same on both the reactant and product sides. This is done by using the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

Q: How do I calculate the amount of a product formed in a chemical reaction?

A: To calculate the amount of a product formed in a chemical reaction, you need to use the concept of stoichiometry and the mole ratio between the reactants and products. This involves calculating the number of moles of the product formed and then multiplying it by the molar mass of the product to get the mass of the product formed.

Q: What is the difference between a balanced equation and an unbalanced equation?

A: A balanced equation is one in which the number of atoms of each element is the same on both the reactant and product sides. An unbalanced equation is one in which the number of atoms of each element is not the same on both the reactant and product sides.

Q: How do I determine the mole ratio between reactants and products in a chemical reaction?

A: To determine the mole ratio between reactants and products in a chemical reaction, you need to look at the coefficients in front of the formulas of the reactants and products in the balanced equation. The coefficients indicate the number of molecules of each reactant and product that participate in the reaction.

Q: What is the law of conservation of mass?

A: The law of conservation of mass states that matter cannot be created or destroyed in a chemical reaction. This means that the total mass of the reactants must be equal to the total mass of the products.

Q: How do I calculate the number of moles of a substance?

A: To calculate the number of moles of a substance, you need to divide the mass of the substance by its molar mass. The molar mass is the mass of one mole of the substance.

Q: What is the difference between a mole and a gram?

A: A mole is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules). A gram is a unit of mass that represents 1/1000 of a kilogram.

Q: How do I convert between moles and grams?

A: To convert between moles and grams, you need to use the molar mass of the substance. The molar mass is the mass of one mole of the substance. You can convert moles to grams by multiplying the number of moles by the molar mass, and you can convert grams to moles by dividing the mass by the molar mass.

Q: What is the significance of stoichiometry in chemistry?

A: Stoichiometry is a crucial concept in chemistry because it allows us to predict the amounts of products formed in a chemical reaction. This is essential in many fields, including chemistry, biology, and engineering.

Q: How do I apply stoichiometry in real-life situations?

A: Stoichiometry is applied in many real-life situations, including:

• Chemical manufacturing: Stoichiometry is used to calculate the amounts of reactants and products required to produce a specific amount of a product.
• Environmental science: Stoichiometry is used to calculate the amounts of pollutants released into the environment.
• Biology: Stoichiometry is used to calculate the amounts of nutrients required by living organisms.
• Engineering: Stoichiometry is used to calculate the amounts of materials required to build structures and machines.

Conclusion

In this article, we have answered some of the most frequently asked questions on stoichiometry and chemical reactions. We have covered topics such as balancing chemical equations, calculating the amount of a product formed, and applying stoichiometry in real-life situations. We hope that this article has provided you with a better understanding of stoichiometry and its significance in chemistry.