The Equation Below Shows Hydrogen Reacting With Oxygen To Produce Water: 2 H 2 + O 2 → 2 H 2 O 2 H_2 + O_2 \rightarrow 2 H_2O 2 H 2 + O 2 → 2 H 2 O If 16 Mol Of Oxygen Were Reacted With Excess Hydrogen Gas, How Many Moles Of Water Would Be Produced?A. 4.0 Mol B. 8.0 Mol C. 16 Mol D.
Introduction
Chemical reactions are the foundation of chemistry, and understanding the stoichiometry of these reactions is crucial in determining the amount of products formed. The equation shows the reaction between hydrogen and oxygen to produce water. In this article, we will explore how to calculate the number of moles of water produced when a certain amount of oxygen is reacted with excess hydrogen gas.
Understanding the Reaction
The given equation indicates that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water. This is a simple example of a chemical reaction, where the reactants are converted into products. In this case, the reactants are hydrogen gas (H2) and oxygen gas (O2), and the product is water (H2O).
Calculating the Number of Moles of Water Produced
To calculate the number of moles of water produced, we need to use the concept of stoichiometry. Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this case, we are given the amount of oxygen gas (16 mol) and we need to find the amount of water produced.
According to the equation, 1 mole of oxygen gas reacts with 2 moles of hydrogen gas to produce 2 moles of water. Therefore, the ratio of oxygen gas to water is 1:2. This means that for every 1 mole of oxygen gas, 2 moles of water are produced.
Applying the Concept of Stoichiometry
To calculate the number of moles of water produced, we can use the following steps:
- Determine the number of moles of oxygen gas reacted.
- Use the ratio of oxygen gas to water to calculate the number of moles of water produced.
In this case, we are given that 16 mol of oxygen gas are reacted. Using the ratio of oxygen gas to water (1:2), we can calculate the number of moles of water produced as follows:
Number of moles of water produced = 2 x Number of moles of oxygen gas reacted = 2 x 16 mol = 32 mol
However, this is not the correct answer. We need to consider the fact that the question states that excess hydrogen gas is present. This means that there is an unlimited supply of hydrogen gas, and the reaction will proceed until all the oxygen gas is consumed.
Considering the Limiting Reactant
In this case, the oxygen gas is the limiting reactant, and the reaction will proceed until all the oxygen gas is consumed. Therefore, the number of moles of water produced will be equal to the number of moles of oxygen gas reacted.
Number of moles of water produced = Number of moles of oxygen gas reacted = 16 mol
Conclusion
In conclusion, when 16 mol of oxygen gas are reacted with excess hydrogen gas, the number of moles of water produced is equal to the number of moles of oxygen gas reacted. This is because the oxygen gas is the limiting reactant, and the reaction will proceed until all the oxygen gas is consumed.
Answer
The correct answer is C. 16 mol.
Discussion
This problem is a classic example of a chemical reaction, where the reactants are converted into products. The concept of stoichiometry is crucial in determining the amount of products formed. In this case, the ratio of oxygen gas to water is 1:2, and the number of moles of water produced is equal to the number of moles of oxygen gas reacted.
Additional Questions
- What is the ratio of hydrogen gas to water in the given equation?
- If 8 mol of oxygen gas are reacted with excess hydrogen gas, how many moles of water will be produced?
- If 32 mol of hydrogen gas are reacted with excess oxygen gas, how many moles of water will be produced?
Answer Key
- The ratio of hydrogen gas to water is 1:1.
- The number of moles of water produced will be 16 mol.
- The number of moles of water produced will be 32 mol.
Q&A: Understanding the Equation of Hydrogen and Oxygen Reaction ================================================================
Introduction
In our previous article, we explored the equation and calculated the number of moles of water produced when a certain amount of oxygen is reacted with excess hydrogen gas. In this article, we will answer some frequently asked questions related to this topic.
Q: What is the ratio of hydrogen gas to water in the given equation?
A: The ratio of hydrogen gas to water in the given equation is 1:1. This means that for every 1 mole of hydrogen gas, 1 mole of water is produced.
Q: If 8 mol of oxygen gas are reacted with excess hydrogen gas, how many moles of water will be produced?
A: To calculate the number of moles of water produced, we need to use the concept of stoichiometry. According to the equation, 1 mole of oxygen gas reacts with 2 moles of hydrogen gas to produce 2 moles of water. Therefore, the ratio of oxygen gas to water is 1:2.
Number of moles of water produced = 2 x Number of moles of oxygen gas reacted = 2 x 8 mol = 16 mol
However, this is not the correct answer. We need to consider the fact that the question states that excess hydrogen gas is present. This means that there is an unlimited supply of hydrogen gas, and the reaction will proceed until all the oxygen gas is consumed.
Number of moles of water produced = Number of moles of oxygen gas reacted = 8 mol
Q: If 32 mol of hydrogen gas are reacted with excess oxygen gas, how many moles of water will be produced?
A: To calculate the number of moles of water produced, we need to use the concept of stoichiometry. According to the equation, 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water. Therefore, the ratio of hydrogen gas to water is 2:2.
Number of moles of water produced = Number of moles of hydrogen gas reacted = 32 mol / 2 = 16 mol
However, this is not the correct answer. We need to consider the fact that the question states that excess oxygen gas is present. This means that there is an unlimited supply of oxygen gas, and the reaction will proceed until all the hydrogen gas is consumed.
Number of moles of water produced = Number of moles of hydrogen gas reacted = 32 mol
Q: What is the limiting reactant in the given equation?
A: The limiting reactant in the given equation is the reactant that is consumed first. In this case, the limiting reactant is oxygen gas.
Q: How can we determine the limiting reactant in a chemical reaction?
A: To determine the limiting reactant in a chemical reaction, we need to compare the mole ratio of the reactants to the mole ratio of the products. The reactant that is consumed first is the limiting reactant.
Q: What is the mole ratio of the reactants to the products in the given equation?
A: The mole ratio of the reactants to the products in the given equation is 2:2:2. This means that for every 2 moles of hydrogen gas, 1 mole of oxygen gas, and 2 moles of water are produced.
Conclusion
In conclusion, understanding the equation of hydrogen and oxygen reaction is crucial in determining the amount of products formed. The concept of stoichiometry is essential in calculating the number of moles of water produced. By answering these frequently asked questions, we hope to provide a better understanding of this topic.
Additional Questions
- What is the ratio of hydrogen gas to water in the given equation?
- If 8 mol of oxygen gas are reacted with excess hydrogen gas, how many moles of water will be produced?
- If 32 mol of hydrogen gas are reacted with excess oxygen gas, how many moles of water will be produced?
- What is the limiting reactant in the given equation?
- How can we determine the limiting reactant in a chemical reaction?
Answer Key
- The ratio of hydrogen gas to water is 1:1.
- The number of moles of water produced will be 8 mol.
- The number of moles of water produced will be 32 mol.
- The limiting reactant is oxygen gas.
- We can determine the limiting reactant by comparing the mole ratio of the reactants to the mole ratio of the products.