Consider The Following Reaction: ${ 2 H_2 + O_2 \rightarrow 2 H_2O }$How Many Moles Of Water Can Be Formed From 2.4 Moles Of ${ H_2 }$ And 2.7 Moles Of ${ O_2 }$?

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Introduction

Chemical reactions involve the transformation of one or more substances into new substances. In this process, the reactants are converted into products, and the number of moles of each substance is crucial in understanding the reaction's outcome. The given reaction, 2H2+O2→2H2O2 H_2 + O_2 \rightarrow 2 H_2O, is a simple example of a chemical reaction where hydrogen gas (H2H_2) reacts with oxygen gas (O2O_2) to form water (H2OH_2O). In this article, we will explore how to determine the number of moles of water that can be formed from a given amount of hydrogen and oxygen.

Understanding the Reaction

The given reaction is a balanced chemical equation, meaning that the number of atoms of each element is the same on both the reactant and product sides. The balanced equation is:

2H2+O2→2H2O2 H_2 + O_2 \rightarrow 2 H_2O

This equation tells us that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water.

Stoichiometry: The Key to Understanding Chemical Reactions

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the use of mole ratios to determine the amount of each substance required or produced in a reaction. In this case, we are interested in finding the number of moles of water that can be formed from a given amount of hydrogen and oxygen.

Calculating the Number of Moles of Water

To calculate the number of moles of water that can be formed, we need to use the mole ratio from the balanced equation. The mole ratio is the ratio of the number of moles of each substance in the balanced equation. In this case, the mole ratio is:

2H2:O2:2H2O=2:1:22 H_2 : O_2 : 2 H_2O = 2 : 1 : 2

This means that for every 2 moles of hydrogen, 1 mole of oxygen is required to produce 2 moles of water.

Step 1: Determine the Limiting Reactant

To determine the number of moles of water that can be formed, we need to identify the limiting reactant. The limiting reactant is the substance that is present in the smallest amount relative to the other substances. In this case, we have 2.4 moles of hydrogen and 2.7 moles of oxygen.

To determine the limiting reactant, we can use the mole ratio from the balanced equation. We can set up a proportion to relate the number of moles of hydrogen to the number of moles of oxygen:

2 moles H21 mole O2=2.4 moles H2x moles O2\frac{2 \text{ moles } H_2}{1 \text{ mole } O_2} = \frac{2.4 \text{ moles } H_2}{x \text{ moles } O_2}

Solving for xx, we get:

x=2.4 moles H22 moles H2×1 mole O2=1.2 moles O2x = \frac{2.4 \text{ moles } H_2}{2 \text{ moles } H_2} \times 1 \text{ mole } O_2 = 1.2 \text{ moles } O_2

Since we have 2.7 moles of oxygen, which is greater than 1.2 moles, oxygen is not the limiting reactant. Therefore, hydrogen is the limiting reactant.

Step 2: Calculate the Number of Moles of Water

Now that we have identified the limiting reactant, we can calculate the number of moles of water that can be formed. We can use the mole ratio from the balanced equation to relate the number of moles of hydrogen to the number of moles of water:

2 moles H22 moles H2O=2.4 moles H2x moles H2O\frac{2 \text{ moles } H_2}{2 \text{ moles } H_2O} = \frac{2.4 \text{ moles } H_2}{x \text{ moles } H_2O}

Solving for xx, we get:

x=2.4 moles H22 moles H2×2 moles H2O=2.4 moles H2Ox = \frac{2.4 \text{ moles } H_2}{2 \text{ moles } H_2} \times 2 \text{ moles } H_2O = 2.4 \text{ moles } H_2O

Therefore, 2.4 moles of water can be formed from 2.4 moles of hydrogen.

Conclusion

In conclusion, the number of moles of water that can be formed from a given amount of hydrogen and oxygen can be determined using the mole ratio from the balanced equation. By identifying the limiting reactant and using the mole ratio, we can calculate the number of moles of water that can be formed. In this case, 2.4 moles of water can be formed from 2.4 moles of hydrogen.

References

  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2002). General chemistry: Principles and modern applications. Prentice Hall.
  • Atkins, P. W., & de Paula, J. (2006). Physical chemistry. Oxford University Press.

Further Reading

  • Stoichiometry: A step-by-step guide
  • Balancing chemical equations
  • Limiting reactants and excess reactants

Glossary

  • Mole ratio: The ratio of the number of moles of each substance in a balanced chemical equation.
  • Limiting reactant: The substance that is present in the smallest amount relative to the other substances in a reaction.
  • Excess reactant: The substance that is present in excess relative to the other substances in a reaction.
    Frequently Asked Questions (FAQs) on Balancing Chemical Equations and Stoichiometry =====================================================================================

Q: What is a balanced chemical equation?

A: A balanced chemical equation is a chemical equation in which the number of atoms of each element is the same on both the reactant and product sides.

Q: Why is balancing a chemical equation important?

A: Balancing a chemical equation is important because it ensures that the law of conservation of mass is obeyed, which means that the total mass of the reactants is equal to the total mass of the products.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to make sure that the number of atoms of each element is the same on both the reactant and product sides. You can do this by adding coefficients (numbers in front of the formulas of the reactants or products) to balance the equation.

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 determine the limiting reactant in a reaction?

A: To determine the limiting reactant in a reaction, you need to compare the mole ratio of the reactants to the mole ratio of the products. The reactant that is present in the smallest amount relative to the other reactants is the limiting reactant.

Q: What is the difference between a limiting reactant and an excess reactant?

A: A limiting reactant is the reactant that is present in the smallest amount relative to the other reactants, while an excess reactant is the reactant that is present in excess relative to the other reactants.

Q: How do I calculate the number of moles of a product in a reaction?

A: To calculate the number of moles of a product in a reaction, you need to use the mole ratio of the reactants to the product. You can do this by setting up a proportion and solving for the number of moles of the product.

Q: What is the mole ratio in a chemical reaction?

A: The mole ratio in a chemical reaction is the ratio of the number of moles of each reactant to the number of moles of each product.

Q: How do I use the mole ratio to calculate the number of moles of a product?

A: To use the mole ratio to calculate the number of moles of a product, you need to set up a proportion and solve for the number of moles of the product.

Q: What is the law of conservation of mass?

A: The law of conservation of mass states that the total mass of the reactants is equal to the total mass of the products in a chemical reaction.

Q: Why is the law of conservation of mass important?

A: The law of conservation of mass is important because it ensures that the total mass of the reactants is equal to the total mass of the products in a chemical reaction.

Q: How do I apply the law of conservation of mass in a chemical reaction?

A: To apply the law of conservation of mass in a chemical reaction, you need to make sure that the total mass of the reactants is equal to the total mass of the products.

Q: What is the difference between a chemical reaction and a physical change?

A: A chemical reaction is a process in which one or more substances are converted into new substances, while a physical change is a process in which a substance changes its state or properties without undergoing a chemical change.

Q: How do I determine if a reaction is a chemical reaction or a physical change?

A: To determine if a reaction is a chemical reaction or a physical change, you need to look for changes in the chemical composition of the substances involved in the reaction.

Q: What is the importance of understanding chemical reactions and stoichiometry?

A: Understanding chemical reactions and stoichiometry is important because it allows us to predict the outcomes of chemical reactions and to design and optimize chemical processes.

Q: How do I apply my knowledge of chemical reactions and stoichiometry in real-world situations?

A: You can apply your knowledge of chemical reactions and stoichiometry in real-world situations by using it to design and optimize chemical processes, to predict the outcomes of chemical reactions, and to solve problems related to chemical reactions and stoichiometry.