Consider The Combustion Reaction For Acetylene:$\[ 2 C_2H_2(l) + 5 O_2(g) \rightarrow 4 CO_2(g) + 2 H_2O(g) \\]If The Acetylene Tank Contains 37.0 Mol Of $C_2H_2$ And The Oxygen Tank Contains 81.0 Mol Of $O_2$, What Is The

Introduction

Chemical reactions are the foundation of chemistry, and understanding the principles behind them is crucial for any aspiring chemist. One of the fundamental concepts in chemistry is the concept of balancing chemical equations. 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. In this article, we will explore the concept of balancing chemical equations and limiting reactants using the combustion reaction of acetylene as a case study.

The Combustion Reaction of Acetylene

The combustion reaction of acetylene is a highly exothermic reaction that releases a significant amount of energy in the form of heat and light. The reaction is as follows:

${ 2 C_2H_2(l) + 5 O_2(g) \rightarrow 4 CO_2(g) + 2 H_2O(g) }$

In this reaction, acetylene ($C_2H_2$) reacts with oxygen ($O_2$) to produce carbon dioxide ($CO_2$) and water ($H_2O$). The reaction is highly dependent on the availability of oxygen, as it is the limiting reactant in this reaction.

Balancing Chemical Equations

Balancing chemical equations is a crucial step in understanding the stoichiometry of a reaction. The balanced equation shows the exact number of moles of each reactant and product involved in the reaction. To balance the equation, we need to ensure that the number of atoms of each element is the same on both the reactant and product sides.

In the case of the combustion reaction of acetylene, we can see that the equation is already balanced. However, to verify this, we can count the number of atoms of each element on both sides of the equation.

Element	Reactant Side	Product Side
C	4	4
H	4	4
O	7	7

As we can see, the number of atoms of each element is the same on both the reactant and product sides, confirming that the equation is balanced.

Limiting Reactants

A limiting reactant is the reactant that is consumed first in a reaction, and it determines the maximum amount of product that can be formed. In the case of the combustion reaction of acetylene, oxygen is the limiting reactant.

To determine the limiting reactant, we need to calculate the number of moles of each reactant required to produce the desired amount of product. In this case, we are given the number of moles of acetylene and oxygen available.

Reactant	Number of Moles
$C_2H_2$	37.0 mol
$O_2$	81.0 mol

To determine the limiting reactant, we need to calculate the number of moles of oxygen required to react with 37.0 mol of acetylene.

From the balanced equation, we can see that 2 mol of $C_2H_2$ react with 5 mol of $O_2$. Therefore, the number of moles of oxygen required to react with 37.0 mol of acetylene is:

${ \frac{5 \text{ mol } O_2}{2 \text{ mol } C_2H_2} \times 37.0 \text{ mol } C_2H_2 = 92.5 \text{ mol } O_2 }$

Since we have only 81.0 mol of oxygen available, oxygen is the limiting reactant.

Calculating the Amount of Product Formed

Now that we have determined the limiting reactant, we can calculate the amount of product formed. In this case, we are interested in calculating the amount of carbon dioxide formed.

From the balanced equation, we can see that 2 mol of $C_2H_2$ produce 4 mol of $CO_2$. Therefore, the number of moles of carbon dioxide formed is:

${ \frac{4 \text{ mol } CO_2}{2 \text{ mol } C_2H_2} \times 37.0 \text{ mol } C_2H_2 = 74.0 \text{ mol } CO_2 }$

Conclusion

In conclusion, balancing chemical equations and determining limiting reactants are crucial steps in understanding the stoichiometry of a reaction. In this article, we have explored the concept of balancing chemical equations and limiting reactants using the combustion reaction of acetylene as a case study. We have shown that the equation is already balanced and that oxygen is the limiting reactant. Finally, we have calculated the amount of product formed, which is 74.0 mol of carbon dioxide.

References

• Atkins, P. W., & de Paula, J. (2010). Physical chemistry. Oxford University Press.
• Chang, R. (2010). Chemistry. McGraw-Hill.
• Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.

Further Reading

• Balancing chemical equations: A step-by-step guide
• Limiting reactants: A comprehensive guide
• Stoichiometry: A fundamental concept in chemistry

Glossary

• Balanced equation: An equation in which the number of atoms of each element is the same on both the reactant and product sides.
• Limiting reactant: The reactant that is consumed first in a reaction, and it determines the maximum amount of product that can be formed.
• Stoichiometry: The study of the quantitative relationships between reactants and products in a chemical reaction.
  Q&A: Balancing Chemical Equations and Limiting Reactants ===========================================================

Introduction

In our previous article, we explored the concept of balancing chemical equations and limiting reactants using the combustion reaction of acetylene as a case study. In this article, we will answer some frequently asked questions related to balancing chemical equations and limiting reactants.

Q: What is a balanced chemical equation?

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

Q: Why is balancing chemical equations important?

A: Balancing chemical equations is important because it allows us to determine the exact number of moles of each reactant and product involved in a reaction. This is crucial for understanding the stoichiometry of a reaction and for predicting the amount of product formed.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to ensure 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 to the reactants and products.

Q: What is a limiting reactant?

A: A limiting reactant is the reactant that is consumed first in a reaction, and it determines the maximum amount of product that can be formed.

Q: How do I determine the limiting reactant?

A: To determine the limiting reactant, you need to calculate the number of moles of each reactant required to produce the desired amount of product. You can do this by using the balanced equation and the number of moles of each reactant available.

Q: What is stoichiometry?

A: Stoichiometry is the study of the quantitative relationships between reactants and products in a chemical reaction.

Q: Why is stoichiometry important?

A: Stoichiometry is important because it allows us to predict the amount of product formed and to determine the limiting reactant.

Q: Can you give an example of how to balance a chemical equation?

A: Yes, let's consider the combustion reaction of methane:

${ CH_4(g) + O_2(g) \rightarrow CO_2(g) + H_2O(g) }$

To balance this equation, we need to ensure that the number of atoms of each element is the same on both the reactant and product sides. We can do this by adding coefficients to the reactants and products:

${ CH_4(g) + 2 O_2(g) \rightarrow CO_2(g) + 2 H_2O(g) }$

Q: Can you give an example of how to determine the limiting reactant?

A: Yes, let's consider the combustion reaction of acetylene:

${ 2 C_2H_2(l) + 5 O_2(g) \rightarrow 4 CO_2(g) + 2 H_2O(g) }$

We are given the number of moles of acetylene and oxygen available:

Reactant	Number of Moles
$C_2H_2$	37.0 mol
$O_2$	81.0 mol

To determine the limiting reactant, we need to calculate the number of moles of oxygen required to react with 37.0 mol of acetylene:

${ \frac{5 \text{ mol } O_2}{2 \text{ mol } C_2H_2} \times 37.0 \text{ mol } C_2H_2 = 92.5 \text{ mol } O_2 }$

Since we have only 81.0 mol of oxygen available, oxygen is the limiting reactant.

Conclusion

In conclusion, balancing chemical equations and determining limiting reactants are crucial steps in understanding the stoichiometry of a reaction. We have answered some frequently asked questions related to balancing chemical equations and limiting reactants, and we have provided examples of how to balance a chemical equation and determine the limiting reactant.

References

• Atkins, P. W., & de Paula, J. (2010). Physical chemistry. Oxford University Press.
• Chang, R. (2010). Chemistry. McGraw-Hill.
• Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.

Further Reading

• Balancing chemical equations: A step-by-step guide
• Limiting reactants: A comprehensive guide
• Stoichiometry: A fundamental concept in chemistry

Glossary

• Balanced equation: An equation in which the number of atoms of each element is the same on both the reactant and product sides.
• Limiting reactant: The reactant that is consumed first in a reaction, and it determines the maximum amount of product that can be formed.
• Stoichiometry: The study of the quantitative relationships between reactants and products in a chemical reaction.