Energetics of Solution | Enthalpy of Solution Explained with Examples | Class 11 Chemistry Lecture скачать в хорошем качестве

Energetics of Solution | Enthalpy of Solution Explained with Examples | Class 11 Chemistry Lecture

#Chemical_energetics #chemistry_class_11 #education #New_first_year_chemistry Lec#67 -8 (Energetics of solution full explained) Playlist with all Chemistry lectures for class 11 new book    • Class 11 chemistry new syllabus 2025 Pakis...   You can get the full chapter in a single PDF without a watermark here. https://umairkhanacademy.com/get-fsc-... Free Chemistry Notes for Chapter 6 https://umairkhanacademy.com/class-11... Energetics of Solution | Enthalpy of Solution Explained with Examples | Class 11 Chemistry Lecture In this lecture, Sir Umair Khan explains the Energetics of Solution (ΔHsol) in detail with examples and easy-to-follow steps. This lecture is specially designed for Class 11 Chemistry (New Book) Chapter 6: Thermochemistry. 🔹 What you will learn in this lecture: Definition of enthalpy of solution (ΔHsol) Difference between exothermic and endothermic solution processes Step-by-step explanation with examples How solute-solute, solvent-solvent, and solute-solvent interactions affect ΔHsol Energetics of dissolving ionic compounds in water Important exam tips for board exams, MDCAT, and ECAT 👨‍🏫 About this lecture: This video is part of the Class 11 Chemistry Chapter 6 series on Thermochemistry. Umair Khan Academy provides simple, exam-focused explanations to help students score high marks. 👉 Don’t forget to Like, Share & Subscribe for more Class 11 and 12 Chemistry lectures. #11th_chemistry_new_book_2025 #chemicalenergetics #BondEnergy #highachieverschemistry #umairkhanacademy #1styearchemistry2025 #chemistry2025 #fscchemistry2025 #sirumairkhan Related Searches: standard conditions. Define standard enthalpy change of reaction, enthalpy change for stoichiometric amounts reacting completely. Define standard enthalpy change of combustion, burning one mole completely in excess oxygen. Define standard enthalpy change of formation, forming one mole of compound from elements. Define standard enthalpy change of atomization, forming one mole of gaseous atoms. Define standard enthalpy change of neutralization, forming one mole of water from acid and alkali. Define bond energy or bond dissociation energy, energy required to break one mole of a bond. Explain the relationship between bond breaking energy, absorbing energy (positive Delta H). Explain the relationship between bond formation energy, releasing energy (negative Delta H). Calculate enthalpy change of reaction, using average bond energies. Calculate the heat transferred, using the relationship q equals m c Delta T. How to measure enthalpy change of a reaction, using a glass calorimeter. Calculate enthalpy change, using the relationship negative m c Delta T over n moles. Define calorie content of food, energy released when food is consumed completely. Outline how enthalpy change relates, to the calorie content of food clearly. Explain Hess’s Law of Heat Summation, total enthalpy change is path independent. Apply Hess’s Law, to calculate enthalpy changes in multi-step reactions. Construct energy cycles or Hess cycles, illustrating enthalpy change routes visually. Calculate Enthalpy of Formation, using Enthalpy of Combustion data. Define dissolution, the process of dissolving a solute in a solvent readily. Define hydration, water molecules surrounding and interacting with solute ions. Define enthalpy of hydration, energy released during ion-dipole force formation. Explain the factors affecting hydration energy magnitude, charge and size of the ion (charge density). Define lattice energy, forming one mole ionic compound from gaseous ions. Explain the factors affecting lattice energy magnitude, charge and size of the ion clearly. Construct Born-Haber Cycles for ionic solids, calculating lattice energy using Hess’s Law. Perform calculations involving energy cycles, linking lattice energy and hydration energy. Define entropy, measure of energy distribution or system disorder. Explain entropy in terms of diffusion, and number of possible arrangements easily. Compare entropy values, based on number of particles, physical state, and hardness. Explain the sign of entropy changes, that occur during state change or gas molecule count change.