Glucose Combustion: Energy Release With 46.233 Mol Oxygen

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Understanding Glucose Combustion

In the fascinating world of chemistry, glucose combustion is a vital process that fuels life itself. It's the chemical reaction where glucose (C6H12O6), a simple sugar, reacts with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O). This reaction is exothermic, meaning it releases energy in the form of heat. The balanced chemical equation for this process is:

C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)

This equation tells us that one mole of solid glucose reacts with six moles of gaseous oxygen to produce six moles of gaseous carbon dioxide and six moles of liquid water. But what about the energy involved? The problem states that this process releases 452.845 kJ per mole of glucose. This value represents the heat of combustion, a crucial piece of information for our calculation.

The heat of combustion, in essence, quantifies the amount of energy liberated when a substance undergoes complete combustion. In this particular instance, each mole of glucose that undergoes combustion liberates 452.845 kilojoules (kJ) of energy. This energy release is a direct consequence of the rearrangement of chemical bonds during the reaction, transitioning from the higher energy state of glucose and oxygen to the lower energy state of carbon dioxide and water. This energetic transformation underscores the significance of glucose as a pivotal fuel source within biological systems, powering various cellular processes and sustaining life's functions.

The significance of glucose combustion extends far beyond the laboratory. It is the primary way our bodies generate energy to perform various functions, from muscle contraction to brain activity. Plants also utilize glucose, produced during photosynthesis, as an energy source. Understanding the energy released during glucose combustion is therefore essential in fields like biology, nutrition, and exercise science. By grasping the quantitative aspects of this reaction, researchers and practitioners can develop informed strategies for optimizing energy expenditure, dietary planning, and athletic performance. Furthermore, the principles of glucose combustion are integral to the study of metabolism, shedding light on the intricate biochemical pathways that govern energy flow within living organisms.

The Question: Energy Released with 46.233 Moles of Oxygen

Now, let's tackle the specific question posed: When 46.233 moles of oxygen react in this way with glucose, what is the total energy released? This is a stoichiometry problem, where we need to use the balanced chemical equation and the heat of combustion to determine the energy produced for a given amount of reactant.

To solve this, we'll use the stoichiometric relationship between oxygen and glucose. The balanced equation shows that 6 moles of oxygen react with 1 mole of glucose. This ratio is our key to converting moles of oxygen to moles of glucose. Once we know the moles of glucose reacted, we can use the heat of combustion (452.845 kJ/mol) to calculate the total energy released. The stoichiometric coefficients in the balanced equation serve as a critical bridge, allowing us to translate the quantity of one substance involved in the reaction to the corresponding quantity of another substance. This fundamental concept underpins quantitative analysis in chemistry, enabling precise calculations of reactant and product amounts, as well as energy changes.

Stoichiometry, at its core, is about understanding the quantitative relationships in chemical reactions. It's the language that allows us to speak precisely about how much of each substance is involved in a chemical transformation. By mastering stoichiometry, we can predict the outcome of reactions, optimize chemical processes, and gain deeper insights into the fundamental laws governing the behavior of matter. This knowledge is invaluable in various fields, from pharmaceutical development to materials science, where precise control over chemical reactions is paramount.

Step-by-Step Calculation

Let's break down the calculation into clear, manageable steps:

  1. Determine the moles of glucose reacted:

    • We know 6 moles of O2 react with 1 mole of glucose.
    • We have 46.233 moles of O2.
    • Moles of glucose = (46.233 moles O2) * (1 mole glucose / 6 moles O2) = 7.7055 moles glucose

    In this initial step, we leverage the stoichiometric ratio derived from the balanced chemical equation. This ratio acts as a conversion factor, enabling us to bridge the gap between the quantity of oxygen involved and the corresponding quantity of glucose that reacts. By carefully applying this conversion, we can accurately determine the number of moles of glucose consumed in the reaction, setting the stage for the subsequent energy calculation. This meticulous approach underscores the importance of stoichiometry in ensuring accurate and reliable results in chemical calculations.

  2. Calculate the total energy released:

    • We know 1 mole of glucose releases 452.845 kJ.
    • We have 7.7055 moles of glucose reacted.
    • Total energy released = (7.7055 moles glucose) * (452.845 kJ / mole glucose) = 3488.59 kJ

    Here, we employ the heat of combustion as a conversion factor to translate the number of moles of glucose combusted into the total energy released. This step directly answers the central question of the problem, quantifying the amount of energy liberated when 46.233 moles of oxygen react with glucose. The result, 3488.59 kJ, represents the magnitude of the exothermic process, highlighting the significant energy output associated with glucose combustion. This energy release is the driving force behind numerous biological processes, underscoring the pivotal role of glucose as a primary fuel source for living organisms.

The Answer

Therefore, when 46.233 moles of oxygen react with glucose in this way, 3488.59 kJ of energy is released.

This calculation demonstrates the power of stoichiometry and the importance of understanding chemical equations. By using the balanced equation and the heat of combustion, we can accurately predict the energy released during a chemical reaction. This ability is crucial in various applications, from designing efficient combustion engines to understanding metabolic processes in living organisms.

Understanding energy release in chemical reactions is crucial for many applications. In industrial settings, this knowledge helps optimize processes like power generation and chemical synthesis. In environmental science, it aids in assessing the impact of combustion processes on air quality. In biochemistry, it's fundamental for understanding how organisms extract energy from food. By mastering these concepts, we gain a deeper understanding of the world around us and the intricate interplay of energy and matter.

Key Takeaways

  • Glucose combustion is an exothermic reaction that releases a significant amount of energy.
  • Stoichiometry is essential for calculating the amount of reactants and products involved in a chemical reaction.
  • The heat of combustion is a crucial value for determining the energy released during combustion.

By mastering these concepts, you can confidently tackle similar chemistry problems and gain a deeper appreciation for the fascinating world of chemical reactions.

In conclusion, understanding the principles of glucose combustion and stoichiometry allows us to calculate the energy released during chemical reactions accurately. This knowledge is vital in various scientific and practical applications, from understanding biological processes to designing efficient energy systems. The problem we solved demonstrates how stoichiometry, combined with the heat of combustion, provides a powerful tool for quantifying energy changes in chemical reactions.

For further learning about stoichiometry and chemical reactions, you can explore resources like Khan Academy's Chemistry Section.