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- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/29%3A_Chemical_Kinetics_II-_Reaction_Mechanisms/29.08%3A_A_Catalyst_Affects_the_Mechanism_and_Activation_EnergyThis page covers the role of catalysts in chemical reactions, highlighting their ability to lower activation energy and increase reaction rates without being consumed. It distinguishes between homogen...This page covers the role of catalysts in chemical reactions, highlighting their ability to lower activation energy and increase reaction rates without being consumed. It distinguishes between homogeneous and heterogeneous catalysts and details mechanisms like Langmuir-Hinshelwood and Eley-Rideal in gas-phase reactions on solid surfaces. The importance of surface area is discussed, along with equations for reaction rates and concentrations.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/26%3A_Chemical_Equilibrium/26.04%3A_Gibbs_Energy_of_a_Reaction_vs._Extent_of_Reaction_is_a_Minimum_at_EquilibriumThis page explains the extent of reaction (\(\xi\)), which quantifies the progress of a chemical reaction. It covers the changes in Gibbs free energy relative to \(\xi\), conditions for spontaneity an...This page explains the extent of reaction (\(\xi\)), which quantifies the progress of a chemical reaction. It covers the changes in Gibbs free energy relative to \(\xi\), conditions for spontaneity and equilibrium, and the relationship between chemical potentials of reactants and products.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.15%3A_Mechanisms_and_Potential_Energy_DiagramsThis page compares roller coasters to chemical reactions, focusing on rate-limiting steps and potential energy diagrams. The ascent of a roller coaster symbolizes the activation energy required for a ...This page compares roller coasters to chemical reactions, focusing on rate-limiting steps and potential energy diagrams. The ascent of a roller coaster symbolizes the activation energy required for a reaction's initial step. It illustrates a two-step reaction with different activation energies, identifying the first step as the rate-limiting one due to its higher activation energy. The overall enthalpy change is defined by the initial and final states, independent of individual steps.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/20%3A_Entropy_and_Free_Energy/20.06%3A_Temperature_and_Free_EnergyThis page discusses the reactions of iron ore and coke producing iron and carbon dioxide at high temperatures. It also explains the decomposition of calcium carbonate into calcium oxide and carbon dio...This page discusses the reactions of iron ore and coke producing iron and carbon dioxide at high temperatures. It also explains the decomposition of calcium carbonate into calcium oxide and carbon dioxide, which requires temperatures exceeding approximately 835°C. Below this temperature, the products are not detectable, but measurable carbon dioxide is produced above 700°C. The quicklime production process leverages the removal of carbon dioxide to favor product formation.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/12%3A_Stoichiometry/12.08%3A_Determining_the_Limiting_ReactantThis page explains how to find the limiting reactant in a chemical reaction, illustrated by the reaction of silver and sulfur to form silver sulfide. It details steps to convert mass to moles, use a b...This page explains how to find the limiting reactant in a chemical reaction, illustrated by the reaction of silver and sulfur to form silver sulfide. It details steps to convert mass to moles, use a balanced equation for mole ratios, and identify excess reactants. In the example provided, silver is the limiting reactant, while sulfur remains in excess. Additionally, it outlines how to calculate the mass of the excess reactant left after the reaction.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.02%3A_Collision_TheoryThis page discusses the financial implications of car damage, highlighting the costs of repairs, particularly in the absence of insurance. It also explains collision theory, which states that for prod...This page discusses the financial implications of car damage, highlighting the costs of repairs, particularly in the absence of insurance. It also explains collision theory, which states that for products to form during reactions, particles must collide with adequate kinetic energy and proper orientation; only effective collisions can rearrange atoms and produce new substances, while ineffective collisions do not result in any changes.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/20%3A_Entropy_and_Free_Energy/20.02%3A_Standard_EntropyThis page discusses geothermal energy sources that utilize steam from geysers to fulfill energy needs. It also explains the concept of entropy, which quantifies molecular motion and has a standard val...This page discusses geothermal energy sources that utilize steam from geysers to fulfill energy needs. It also explains the concept of entropy, which quantifies molecular motion and has a standard value at absolute zero. As temperature increases, entropy rises, and the page details how to calculate entropy changes for reactions like water vaporization and liquid formation. It emphasizes that reactions can still be favorable despite a decrease in entropy when they are exothermic.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/26%3A_Chemical_Equilibrium/26.07%3A_The_van_'t_Hoff_EquationThis page explains the Gibbs-Helmholtz equation's significance in analyzing how the equilibrium constant \(K\) varies with temperature in chemical reactions, emphasizing the connection to the reaction...This page explains the Gibbs-Helmholtz equation's significance in analyzing how the equilibrium constant \(K\) varies with temperature in chemical reactions, emphasizing the connection to the reaction's enthalpy \(ΔH^o\).
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Chemistry_Basics/LavoisierUnlike the Greek philosophers, he understood that this is a physical change, not a chemical change, and he has a good submicroscopic-scale intuition of what's happening: the particles of the material ...Unlike the Greek philosophers, he understood that this is a physical change, not a chemical change, and he has a good submicroscopic-scale intuition of what's happening: the particles of the material don't change, they just get further apart. For instance, in the experiment we just described, he measured the volume of gas in the bell jar, before and after the reaction, but noted that after the reaction, you must wait until the temperature returns to what it was when you measured originally.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/18%3A_Kinetics/18.09%3A_Order_of_ReactionThis page discusses the impact of forest fires on ecosystems, emphasizing the relationship between fire severity and dry plant material. It also explains chemical kinetics, focusing on first-order rea...This page discusses the impact of forest fires on ecosystems, emphasizing the relationship between fire severity and dry plant material. It also explains chemical kinetics, focusing on first-order reactions, which depend on the concentration of one reactant, and second-order reactions involving multiple reactants. The importance of conducting experiments to establish rate laws and reaction orders is highlighted.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.15%3A_Hess's_Law_of_Heat_SummationThis page explains the complexities involved in calculating the energy associated with operating an acetylene torch. It highlights the use of Hess's law to determine enthalpy changes indirectly throug...This page explains the complexities involved in calculating the energy associated with operating an acetylene torch. It highlights the use of Hess's law to determine enthalpy changes indirectly through combustion reactions. By analyzing the combustion of carbon, hydrogen, and acetylene, the heat of formation for acetylene is found to be 228.3 kJ, which signifies that the reaction is endothermic and absorbs heat.
