Moles Of Carbon Dioxide Produced Propane Combustion

Chemical reactions are the heart of chemistry, and understanding them requires a solid grasp of stoichiometry, the study of the quantitative relationships between reactants and products in chemical reactions. A crucial concept in stoichiometry is the mole, a unit of measurement for the amount of a substance. This article delves into a specific stoichiometric problem: determining the number of moles of carbon dioxide produced when 3.00 moles of oxygen react completely in the combustion of propane. This exploration will not only provide the answer but also illuminate the underlying principles of mole ratios and balanced chemical equations. We will walk through the balanced equation, which serves as the foundation for our calculations, and then meticulously apply mole ratios to arrive at the solution. By the end of this discussion, you will have a clearer understanding of how to approach similar stoichiometric problems and appreciate the quantitative nature of chemical reactions.

The Balanced Chemical Equation: A Foundation for Stoichiometry

The cornerstone of any stoichiometric calculation is the balanced chemical equation. This equation provides the precise ratio in which reactants combine and products are formed. For the combustion of propane (${C_3H_8}$), the balanced equation is:

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

This equation tells us that one molecule of propane reacts with five molecules of oxygen to produce three molecules of carbon dioxide and four molecules of water. However, in chemistry, we typically deal with macroscopic quantities, which are best expressed in moles. Therefore, we can interpret the equation as:

• 1 mole of propane reacts with 5 moles of oxygen
• producing 3 moles of carbon dioxide
• and 4 moles of water

The coefficients in front of each chemical formula represent the number of moles of that substance involved in the reaction. These coefficients are the key to determining mole ratios, which are essential for solving stoichiometric problems. To fully appreciate the significance of a balanced equation, consider what it represents at a fundamental level. It embodies the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. By balancing the equation, we ensure that the number of atoms of each element is the same on both sides of the equation. This balance is crucial for accurate quantitative analysis. For example, in our equation, we have 3 carbon atoms, 8 hydrogen atoms, and 10 oxygen atoms on both the reactant and product sides. This atomic balance is the foundation upon which we build our mole ratios and subsequent calculations. Understanding the balanced chemical equation is not merely about memorizing coefficients; it's about grasping the fundamental principles that govern chemical transformations. This understanding allows us to predict the outcomes of reactions, optimize reaction conditions, and design new chemical processes. In the context of our problem, the balanced equation provides the crucial link between the amount of oxygen consumed and the amount of carbon dioxide produced. This link, expressed as a mole ratio, is the key to unlocking the solution.

Applying Mole Ratios to Determine Carbon Dioxide Production

The mole ratio is a conversion factor derived from the coefficients of the balanced chemical equation. It allows us to convert between the moles of one substance and the moles of another substance in a chemical reaction. In our case, we are interested in the relationship between oxygen (${O_2}$) and carbon dioxide (${CO_2}$). From the balanced equation:

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

We can see that 5 moles of oxygen produce 3 moles of carbon dioxide. This gives us the mole ratio:

${ \frac{3 \text{ moles } CO_2}{5 \text{ moles } O_2} }$

This ratio is the key to solving our problem. We are given that 3.00 moles of oxygen react completely. To find the moles of carbon dioxide produced, we multiply the given moles of oxygen by the mole ratio:

${ 3.00 \text{ moles } O_2 \times \frac{3 \text{ moles } CO_2}{5 \text{ moles } O_2} = 1.80 \text{ moles } CO_2 }$

Therefore, when 3.00 moles of oxygen react completely, 1.80 moles of carbon dioxide are produced. To further illustrate the power of mole ratios, let's consider a slightly different scenario. Suppose we wanted to determine how many moles of propane would be required to react completely with 3.00 moles of oxygen. From the balanced equation, we know that 1 mole of propane reacts with 5 moles of oxygen. This gives us a different mole ratio:

${ \frac{1 \text{ mole } C_3H_8}{5 \text{ moles } O_2} }$

Multiplying the given moles of oxygen by this mole ratio, we get:

${ 3.00 \text{ moles } O_2 \times \frac{1 \text{ mole } C_3H_8}{5 \text{ moles } O_2} = 0.60 \text{ moles } C_3H_8 }$

This shows that 0.60 moles of propane are required to react completely with 3.00 moles of oxygen. These examples highlight the versatility of mole ratios in solving stoichiometric problems. By carefully analyzing the balanced chemical equation and extracting the appropriate mole ratios, we can quantitatively relate the amounts of reactants and products involved in a chemical reaction. This ability is fundamental to many aspects of chemistry, from laboratory experiments to industrial chemical processes. Understanding the mole concept and how to apply mole ratios is a cornerstone of stoichiometric calculations. It allows chemists to predict the amount of product formed from a given amount of reactant, or vice versa, and is essential for designing and optimizing chemical reactions.

The Answer and Its Significance

Based on our calculations, the correct answer is:

B. 1.80 moles

This answer signifies that for every 3.00 moles of oxygen that react in the combustion of propane, 1.80 moles of carbon dioxide are produced. This quantitative relationship is crucial in various applications, such as:

• Environmental Chemistry: Understanding the amount of carbon dioxide produced from combustion reactions is vital for assessing the impact on greenhouse gas emissions and climate change.
• Industrial Chemistry: In industrial processes, precise control over reactant ratios and product yields is essential for efficiency and cost-effectiveness. Stoichiometry plays a key role in optimizing these processes.
• Analytical Chemistry: Stoichiometric calculations are used to determine the composition of substances and the purity of chemical samples.

The ability to accurately predict the amount of product formed from a given amount of reactant is a cornerstone of chemistry. It allows us to design and control chemical reactions for a variety of purposes. The problem we solved is a fundamental example of how stoichiometry is applied in practice. By understanding the mole concept, balanced chemical equations, and mole ratios, we can make quantitative predictions about chemical reactions. This ability is essential for anyone working in chemistry or related fields. The significance of this problem extends beyond the specific reaction of propane combustion. The principles we applied are applicable to a wide range of chemical reactions. Whether it's synthesizing new materials, analyzing environmental samples, or developing new energy technologies, stoichiometry is an indispensable tool for chemists and engineers. The ability to translate between moles of different substances is critical for understanding chemical transformations and their implications.

In conclusion, this exercise in calculating the moles of carbon dioxide produced in propane combustion demonstrates the power and importance of stoichiometry. By carefully applying the concepts of balanced equations and mole ratios, we can accurately predict the quantitative outcomes of chemical reactions. This understanding is essential for a wide range of applications in chemistry and related fields. Mastering stoichiometry is not just about solving problems; it's about developing a fundamental understanding of the quantitative nature of chemistry.