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80bcae78-2071-43b4-96d0-fd8ac4a28430 The Maxwell-Boltzman curve can be used to explain the effect of temperature on reaction rates. Summary

535747cc-4a12-4946-8602-234cd0bca792 Solving Problems Summary To determine the energy released or required

< Back Reaction kinetics Previous Next 🔬 Chapter 9: Rates of Reaction 🔬 Learning Outcomes 🎯: Understand reaction kinetics and the factors affecting the rates of chemical reactions. Recognize the role of surface area, concentration, temperature, and catalysts in reaction rates. Understand the concept of activation energy and its role in determining the rate of reaction. Differentiate between homogeneous and heterogeneous catalysts. Understand the Boltzmann distribution of molecular energies and how it changes with temperature. Factors Affecting Rate of Reaction 📈: Surface Area : Finely divided solids have a larger surface area, leading to more frequent collisions and a faster reaction rate. Concentration and Pressure : Higher concentration or pressure leads to more frequent collisions between reactant molecules, increasing the reaction rate. Temperature : At higher temperatures, molecules have more kinetic energy, leading to more frequent and successful collisions. Catalysts : Catalysts increase the rate of reaction by providing an alternative reaction pathway with a lower activation energy. Activation Energy ⚡: Activation energy is the minimum energy required by colliding particles for a reaction to occur. It acts as a barrier to reaction, and only particles with energy greater than the activation energy can react. Boltzmann Distribution 📊: The Boltzmann distribution represents the number of molecules in a sample with particular energies. At higher temperatures, the distribution changes, showing that more molecules have energy greater than the activation energy, leading to an increase in reaction rate. Catalysis 🧪: Catalysts lower the activation energy, allowing a greater proportion of molecules to have sufficient energy to react. Homogeneous catalysts are in the same phase as the reactants, while heterogeneous catalysts are in a different phase. Enzymes are biological catalysts that provide an alternative reaction pathway of lower activation energy.

94b25da5-79f4-4454-a3cd-3b49473275b2 8. Any reaction or process that releases heat energy Exothermic Summary

efd481a4-b0ce-48ea-aaa8-890c788a5151 dm³ Summary A unit of volume equal to one cubic decimeter, equivalent to 1 liter.

04ce2f71-3e30-4a65-b7a6-d360c2a2add9 < Back Previous Next Stoichiometry Next Topic

8ab8f71e-1a76-468f-9332-0a283163e5ec Find heat involved with given mass of reactant/product from H Summary Finding the heat involved with a given mass of reactant or product from ΔH (enthalpy change) is an important aspect of thermochemistry. It allows us to determine the amount of heat transferred during a chemical reaction, based on the known enthalpy change and the mass of the reactant or product. The heat involved (q) can be calculated using the equation q = ΔH * m, where q represents the heat involved, ΔH is the enthalpy change, and m is the mass of the reactant or product. To use this equation, we need to know the value of ΔH, which can be obtained from experimental data or calculated using thermochemical equations. Additionally, we need to know the mass (m) of the reactant or product involved in the reaction. For example, let's consider the combustion of methane (CH4), where the enthalpy change (ΔH) is known to be -890 kJ/mol. If we have 10 grams of methane, we can calculate the heat involved as follows: q = ΔH * m = -890 kJ/mol * (10 g / 16 g/mol) = -556.25 kJ Therefore, in this case, the heat involved with 10 grams of methane in the combustion reaction is approximately -556.25 kJ. It's important to note that the sign of the enthalpy change (ΔH) indicates the direction of heat transfer. A negative ΔH value represents an exothermic reaction, where heat is released, while a positive ΔH value represents an endothermic reaction, where heat is absorbed. It's crucial to ensure that the units of enthalpy change (ΔH) and mass (m) are consistent in the calculation. If the enthalpy change is given in kilojoules per mole (kJ/mol), the mass should be in moles as well. By using the equation q = ΔH * m, we can determine the heat involved with a given mass of reactant or product in a reaction. This calculation allows us to understand the energy changes associated with chemical reactions and provides valuable insights into the heat flow within a system. In summary, finding the heat involved with a given mass of reactant or product involves using the equation q = ΔH * m, where q represents the heat involved, ΔH is the enthalpy change, and m is the mass of the reactant or product. By multiplying the enthalpy change by the mass, we can calculate the amount of heat transferred. Understanding and calculating the heat involved are essential in studying and analyzing energy changes in chemical reactions.

3d51ee66-6dbf-4730-90eb-260b9e9ffd8b Subscript Summary The number used after a chemical symbol to indicate the number of atoms present per molecule

⚛️ Lesson 4 ⚛️ < Back Atomic Structure Lesson 4 ⚛️ Lesson 4 ⚛️ Explore the world of atomic and ionic radii in this visually enhanced quiz. Discover the patterns of atomic size across the Periodic Table and the changes in ionic radius when atoms gain or lose electrons. Unveil the secrets of the microcosm, one atom at a time! Previous Next ⚛️ 1.1.4 Atomic & Ionic Radius ⚛️ 💥🔬 Navigating the Universe of Atoms: Atomic & Ionic Radii 🔬💥 🌌 Measuring Atomic Size: Atomic Radius 🌌 When we think of the atomic radius, we're actually measuring the size of an atom. 📏 But how? Imagine taking two atoms of the same type, say two hydrogen atoms, bonding them together, and then measuring the distance between their nuclei. 📍📍 The atomic radius is half of this distance. 🧪 But atoms are not all the same size! Just like cities across a country, they show trends across the Periodic Table. 🗺️💡 📉 As you travel across each Period (left to right), atomic radii generally decrease. Why? Well, as you move across, the atomic number increases—meaning more protons. More protons = stronger pull on electrons = smaller atoms. 🔄 📈 On the other hand, as you journey down each Group (top to bottom), atomic radii generally increase. Here, we have more electron shells, which "shield" outermost electrons from the pull of the nucleus—leading to bigger atoms! 🔄 And what about that big jump in size between a noble gas at the end of a period and the alkali metal at the beginning of the next? It's all about the extra shell! More shells = more shielding = larger atomic radius! 💥 🌠 Examining Ion Sizes: Ionic Radius 🌠 The ionic radius, on the other hand, measures the size of an ion—a charged atom. Just like atomic radius, ionic radius also follows certain patterns! 🧩🔍 🔽 If an atom gains extra electrons to become a negatively charged ion (anion), its ionic radius increases. Why? The extra electrons are further from the nucleus and are loosely held, which increases the size. 🔄 🔼 If an atom loses electrons to become a positively charged ion (cation), its ionic radius decreases. Here, the remaining electrons are pulled in tighter by the nucleus, resulting in a smaller ion. 🔄 So, atomic and ionic radii offer a sort of "map" to the universe of atoms and ions. By understanding these trends, you're not just studying chemistry—you're discovering the unseen landscape of the microcosm, one atom (or ion) at a time! 💥🌌

AMS and Periodic 1 Term 2 Revision Term 2 Week 5 AMS and Periodic 1 Term 2 Revision Welcome To Lesson Summary , this lesson included Revision on week 4 and 5 Term 2 plus revision on chapter 5 Course revision questions for periodic 1 term 2 Grade 9 SABIS

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