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6: Quantities in Chemical Reactions

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    So far, we have talked about chemical reactions in terms of individual atoms and molecules. Although this works, most of the reactions occurring around us involve much larger amounts of chemicals. Even a tiny sample of a substance will contain millions, billions, or a hundred billion billions of atoms and molecules. How do we compare amounts of substances to each other in chemical terms when it is so difficult to count to a hundred billion billion? Actually, there are ways to do this, which we will explore in this chapter. In doing so, we will increase our understanding of stoichiometry, which is the study of the numerical relationships between the reactants and the products in a balanced chemical reaction.

    • 6.0: Prelude to Quantities in Chemical Reactions
      This page summarizes Antoine Lavoisier's experiment on water composition, illustrating the law of conservation of matter. He found that the initial mass of water and charcoal equals the final mass of carbonic acid and gas, highlighting the significance of precise measurements in chemistry and other fields. Errors in measurement can have serious implications, impacting areas such as nursing, food production, and manufacturing quality control.
    • 6.1: The Mole
      This page explains the mole unit in chemistry, defined as 6.022 × 10^23 entities (Avogadro's number), and its significance in converting between macroscopic quantities and atomic or molecular counts. It illustrates consistent mass ratios and provides examples on calculating the number of atoms or formula units in a sample. Overall, it emphasizes that one mole contains 6.022 × 10^23 units, whether atoms, molecules, or formula units.
    • 6.2: Atomic and Molar Masses
      This page explains the concept of moles, focusing on Avogadro's number (\(6.022 \times 10^{23}\)) and its link to atomic and gram mass units. It discusses that one mole of a substance corresponds to its atomic mass in grams and provides examples of converting moles to mass. Molar mass is defined as grams per mole (g/mol), highlighting the importance of meticulous atom counting in chemical formulas for accurate molar mass determinations, which are essential for conversions between moles and grams.
    • 6.3: Mole-Mass Conversions
      This page emphasizes the importance of converting between mass and mole units in chemistry using molar mass as a key factor for accurate measurements, particularly in experiments. It also discusses dietary minerals, focusing on chromium, which is required in small amounts but essential for health; deficiencies can lead to serious issues like diabetes, while excessive intake poses risks.
    • 6.4: Mole-Mole Relationships in Chemical Reactions
      This page covers balanced chemical reactions and their role in determining molar relationships between substances. It explains how coefficients in balanced equations represent molecules and molar amounts, detailing the ratios used to connect reactants and products. The text introduces stoichiometry as the study of these relationships, providing examples and an exercise to practice calculating moles of reactants needed in a reaction.
    • 6.5: Mole-Mass and Mass-Mass Problems
      This page explores stoichiometry in chemical reactions, emphasizing mole-mass and mass-mass calculations through balanced equations, supported by examples. It also discusses the Pacific yew tree's role in Taxol production and the challenges of lab synthesis, which is complex and inefficient. With significant demand for Taxol to treat ovarian cancer, improving synthesis efficiency is crucial to minimize waste and enhance accessibility to this vital treatment.
    • 6.E: Quantities in Chemical Reactions (Exercise)
      This page discusses exercises on the mole concept, covering definitions, calculations for determining moles and molar masses, and mole-mass conversions. It emphasizes the role of balanced chemical equations in maintaining molar ratios and conservation of matter. Furthermore, it includes practical exercises on various chemical reactions, mass-mass calculations, and solutions for determining moles and masses of reactants and products, with detailed answers provided for each exercise.
    • 6.S: Quantities in Chemical Reactions (Summary)
      This page covers fundamental chemistry concepts such as chemical reactions, moles, and stoichiometry. It explains the mole as a unit connecting mass to atomic mass, emphasizes the Law of Conservation of Mass through balanced equations, and introduces Collision Theory and Enthalpy regarding energy changes in reactions. Factors influencing reaction rates, including activation energy and catalysts, are also discussed, along with equilibrium and Le Chatelier's principle.
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