{ C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O \}$If 100.0 Grams Of ${$ C_3H_8 \$}$ Burns, How Many Moles Of Carbon Dioxide Will Form?Given: - ${$ C = 12.001 \$}$Target: Calculate The Moles Of ${$ CO_2 \$}$ Formed. Note:

Introduction

Chemical reactions involve the transformation of one or more substances into new substances. In this article, we will focus on a specific chemical reaction where propane (${ C_3H_8 }$) burns in the presence of oxygen (${ O_2 }$) to form carbon dioxide (${ CO_2 }$) and water (${ H_2O }$). The balanced chemical equation for this reaction is:

${ C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O }$

Understanding the Chemical Equation

The given chemical equation represents the combustion of propane in oxygen to produce carbon dioxide and water. The equation is balanced, meaning that the number of atoms of each element is the same on both the reactant and product sides. The coefficients in front of the formulas of the reactants and products indicate the number of molecules of each substance involved in the reaction.

Calculating Moles of Carbon Dioxide Formed

To calculate the number of moles of carbon dioxide formed when 100.0 grams of propane burns, we need to follow a step-by-step approach.

Step 1: Calculate the Number of Moles of Propane

First, we need to calculate the number of moles of propane (${ C_3H_8 }$) present in 100.0 grams. The molar mass of propane is the sum of the atomic masses of its constituent atoms:

${ M_{C_3H_8} = 3 \times M_C + 8 \times M_H }$

${ M_{C_3H_8} = 3 \times 12.001 + 8 \times 1.008 }$

${ M_{C_3H_8} = 36.003 + 8.064 }$

${ M_{C_3H_8} = 44.067 \, g/mol }$

Now, we can calculate the number of moles of propane using the formula:

${ n = \frac{m}{M} }$

where ${ n }$ is the number of moles, ${ m }$ is the mass of the substance, and ${ M }$ is the molar mass.

${ n_{C_3H_8} = \frac{100.0 \, g}{44.067 \, g/mol} }$

${ n_{C_3H_8} = 2.268 \, mol }$

Step 2: Calculate the Number of Moles of Carbon Dioxide

According to the balanced chemical equation, 1 mole of propane produces 3 moles of carbon dioxide. Therefore, we can calculate the number of moles of carbon dioxide formed by multiplying the number of moles of propane by 3:

${ n_{CO_2} = 3 \times n_{C_3H_8} }$

${ n_{CO_2} = 3 \times 2.268 \, mol }$

${ n_{CO_2} = 6.804 \, mol }$

Conclusion

In this article, we calculated the number of moles of carbon dioxide formed when 100.0 grams of propane burns in the presence of oxygen. We followed a step-by-step approach, first calculating the number of moles of propane present in 100.0 grams, and then using the stoichiometry of the reaction to determine the number of moles of carbon dioxide formed. The result shows that 6.804 moles of carbon dioxide are produced when 100.0 grams of propane burns.

Discussion

The calculation of moles of carbon dioxide formed in a chemical reaction is an essential concept in chemistry. It helps us understand the quantitative relationships between reactants and products in a reaction. In this article, we applied the concept of stoichiometry to calculate the number of moles of carbon dioxide formed when propane burns in oxygen. This type of calculation is crucial in various fields, including chemistry, chemical engineering, and environmental science.

Limitations

While the calculation of moles of carbon dioxide formed is a straightforward process, there are some limitations to consider. For example, the calculation assumes that the reaction is carried out under ideal conditions, with no losses or side reactions. In reality, the reaction may not be 100% efficient, and some of the propane may not burn completely. Additionally, the calculation does not take into account the presence of any catalysts or inhibitors that may affect the reaction rate or yield.

Future Directions

The calculation of moles of carbon dioxide formed can be applied to a wide range of chemical reactions, including those involving other hydrocarbons, alcohols, and other organic compounds. Future research could focus on developing more accurate models for predicting the yield and selectivity of chemical reactions, as well as exploring new catalysts and reaction conditions to improve the efficiency and sustainability of chemical processes.

References

• CRC Handbook of Chemistry and Physics, 97th ed., CRC Press, 2016.
• Chemical Thermodynamics, 2nd ed., John Wiley & Sons, 2013.
• Physical Chemistry: A Molecular Approach, 3rd ed., W.H. Freeman and Company, 2015.
  

Introduction

In our previous article, we discussed the calculation of moles of carbon dioxide formed when propane burns in oxygen. In this article, we will address some of the most frequently asked questions (FAQs) related to this topic.

Q1: What is the molar mass of propane?

A1: The molar mass of propane (${ C_3H_8 }$) is 44.067 g/mol.

Q2: How do I calculate the number of moles of propane present in 100.0 grams?

A2: To calculate the number of moles of propane, you can use the formula:

${ n = \frac{m}{M} }$

where ${ n }$ is the number of moles, ${ m }$ is the mass of the substance, and ${ M }$ is the molar mass.

In this case, the number of moles of propane is:

${ n_{C_3H_8} = \frac{100.0 \, g}{44.067 \, g/mol} }$

${ n_{C_3H_8} = 2.268 \, mol }$

Q3: How do I calculate the number of moles of carbon dioxide formed?

A3: According to the balanced chemical equation, 1 mole of propane produces 3 moles of carbon dioxide. Therefore, you can calculate the number of moles of carbon dioxide formed by multiplying the number of moles of propane by 3:

${ n_{CO_2} = 3 \times n_{C_3H_8} }$

${ n_{CO_2} = 3 \times 2.268 \, mol }$

${ n_{CO_2} = 6.804 \, mol }$

Q4: What are some common sources of error in calculating moles of carbon dioxide formed?

A4: Some common sources of error in calculating moles of carbon dioxide formed include:

• Incorrect molar mass of propane: Make sure to use the correct molar mass of propane (44.067 g/mol).
• Incorrect number of moles of propane: Double-check your calculation to ensure that you have the correct number of moles of propane.
• Incorrect stoichiometry: Make sure to use the correct stoichiometry (1 mole of propane produces 3 moles of carbon dioxide).
• Presence of impurities: If the propane sample contains impurities, it may affect the calculation.

Q5: How can I improve the accuracy of my calculations?

A5: To improve the accuracy of your calculations, make sure to:

• Use high-quality data: Use reliable sources of data, such as the CRC Handbook of Chemistry and Physics.
• Double-check your calculations: Verify your calculations to ensure that you have the correct answers.
• Consider the presence of impurities: If the propane sample contains impurities, take this into account when calculating the number of moles of carbon dioxide formed.
• Use a calculator or computer program: Consider using a calculator or computer program to perform the calculations, as this can help reduce errors.

Q6: What are some real-world applications of calculating moles of carbon dioxide formed?

A6: Calculating moles of carbon dioxide formed has many real-world applications, including:

• Environmental science: Understanding the amount of carbon dioxide formed during combustion reactions is essential for predicting the impact of human activities on the environment.
• Chemical engineering: Calculating moles of carbon dioxide formed is crucial for designing and optimizing chemical processes, such as those used in the production of fuels and chemicals.
• Energy production: Understanding the amount of carbon dioxide formed during combustion reactions is essential for predicting the efficiency and sustainability of energy production systems.

Conclusion

In this article, we addressed some of the most frequently asked questions (FAQs) related to calculating moles of carbon dioxide formed. We hope that this article has provided you with a better understanding of this important topic and has helped you to improve your skills in calculating moles of carbon dioxide formed.