Calculating the Number of Moles of Each Reactant

Oct 13, 2025 by recoveryshake.com 85 views

11. Hydrogen Gas Reacts with Oxygen Gas to Form Water: A Comprehensive Analysis

Hydrogen gas $\left( H_2 \right)$ and oxygen gas $\left( O_2 \right)$ are two highly reactive gases that can combine to form water according to the reaction: $2 H_2 + O_2 \rightarrow 2 H_2O$ . This reaction is a fundamental process in chemistry that has numerous applications in various fields, including energy production, industrial processes, and environmental science. In this article, we will delve into the details of this reaction, exploring the stoichiometry, limiting reactant, and yield of the reaction.

The balanced chemical equation for the reaction between hydrogen gas and oxygen gas is: $2 H_2 + O_2 \rightarrow 2 H_2O$ . This equation indicates that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water. The coefficients in the equation represent the mole ratio of the reactants and products.

To determine the limiting reactant, we need to calculate the number of moles of each reactant required to react with the given amount of the other reactant. Let's assume we start with 6.0 moles of $H_2$ and 2.0 moles of $O_2$ .

Calculating the Number of Moles of Each Reactant

To calculate the number of moles of each reactant required to react with the given amount of the other reactant, we can use the mole ratio from the balanced equation.

For hydrogen gas: $2 H_2 + O_2 \rightarrow 2 H_2O$ $2$ moles of $H_2$ react with $1$ mole of $O_2$

To find the number of moles of $O_2$ required to react with 6.0 moles of $H_2$ , we can divide the number of moles of $H_2$ by 2: $6.0$ moles of $H_2$ $\div$ $2$ = $3.0$ moles of $O_2$

Similarly, to find the number of moles of $H_2$ required to react with 2.0 moles of $O_2$ , we can multiply the number of moles of $O_2$ by 2: $2.0$ moles of $O_2$ $\times$ $2$ = $4.0$ moles of $H_2$

Determining the Limiting Reactant

Based on the calculations above, we can see that 6.0 moles of $H_2$ require 3.0 moles of $O_2$ to react, while 2.0 moles of $O_2$ require 4.0 moles of $H_2$ to react. Since we have 6.0 moles of $H_2$ and only 2.0 moles of $O_2$ , the oxygen gas is the limiting reactant.

Calculating the Yield of the Reaction

Now that we have determined the limiting reactant, we can calculate the yield of the reaction. The yield is the amount of product formed per unit amount of limiting reactant.

In this case, the limiting reactant is oxygen gas, and the amount of oxygen gas available is 2.0 moles. According to the balanced equation, 1 mole of oxygen gas produces 2 moles of water. Therefore, the yield of the reaction is: $2.0$ moles of $O_2$ $\times$ $2$ = $4.0$ moles of $H_2O$

In conclusion, the reaction between hydrogen gas and oxygen gas to form water is a fundamental process in chemistry that has numerous applications in various fields. By analyzing the stoichiometry of the reaction, we can determine the limiting reactant and calculate the yield of the reaction. In this case, the oxygen gas is the limiting reactant, and the yield of the reaction is 4.0 moles of water.

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling

Hydrogen Gas: Properties, Production, and Applications
Oxygen Gas: Properties, Production, and Applications
Water: Properties, Production, and Applications
11. Hydrogen Gas Reacts with Oxygen Gas to Form Water: A Comprehensive Analysis

Q: What is the balanced chemical equation for the reaction between hydrogen gas and oxygen gas?

A: The balanced chemical equation for the reaction between hydrogen gas and oxygen gas is: $2 H_2 + O_2 \rightarrow 2 H_2O$ .

Q: What is the mole ratio of hydrogen gas to oxygen gas in the balanced equation?

A: The mole ratio of hydrogen gas to oxygen gas in the balanced equation is 2:1, meaning that 2 moles of hydrogen gas react with 1 mole of oxygen gas.

Q: How do you determine the limiting reactant in a chemical reaction?

A: To determine the limiting reactant, you need to calculate the number of moles of each reactant required to react with the given amount of the other reactant. The reactant that is present in the smallest amount is the limiting reactant.

Q: What is the limiting reactant in the reaction between hydrogen gas and oxygen gas?

A: In the reaction between hydrogen gas and oxygen gas, the oxygen gas is the limiting reactant.

Q: How do you calculate the yield of a chemical reaction?

A: To calculate the yield of a chemical reaction, you need to determine the amount of product formed per unit amount of limiting reactant.

Q: What is the yield of the reaction between hydrogen gas and oxygen gas?

A: The yield of the reaction between hydrogen gas and oxygen gas is 4.0 moles of water.

Q: What are some common applications of the reaction between hydrogen gas and oxygen gas?

A: Some common applications of the reaction between hydrogen gas and oxygen gas include:

Energy production: Hydrogen gas can be used as a clean and renewable energy source.
Industrial processes: Hydrogen gas is used in various industrial processes, such as the production of chemicals and fuels.
Environmental science: The reaction between hydrogen gas and oxygen gas is an important process in the Earth's atmosphere, where it helps to regulate the concentration of oxygen and hydrogen.

Q: What are some safety precautions that should be taken when working with hydrogen gas and oxygen gas?

A: Some safety precautions that should be taken when working with hydrogen gas and oxygen gas include:

Handling the gases in a well-ventilated area to prevent the buildup of flammable gases.
Using proper equipment and safety gear, such as gloves and goggles, to prevent injury.
Following proper procedures for handling and storing the gases to prevent accidents.

Q: What are some common mistakes that can be made when working with hydrogen gas and oxygen gas?

A: Some common mistakes that can be made when working with hydrogen gas and oxygen gas include:

Not following proper safety procedures, which can lead to accidents and injuries.
Not handling the gases properly, which can lead to contamination and equipment damage.
Not understanding the properties and behavior of the gases, which can lead to incorrect calculations and predictions.

In conclusion, the reaction between hydrogen gas and oxygen gas to form water is a fundamental process in chemistry that has numerous applications in various fields. By understanding the stoichiometry of the reaction, we can determine the limiting reactant and calculate the yield of the reaction. Additionally, by following proper safety procedures and understanding the properties and behavior of the gases, we can minimize the risks associated with working with hydrogen gas and oxygen gas.

Chemistry: An Atoms First Approach, by Steven S. Zumdahl
General Chemistry: Principles and Modern Applications, by Linus Pauling

Hydrogen Gas: Properties, Production, and Applications
Oxygen Gas: Properties, Production, and Applications
Water: Properties, Production, and Applications