Chapter 6 (Lec 61 -2) Standard enthalpy changes + Quick check 6.1 & 6.2 #sirumairkhan chemistry 11

#chemistry #chemistry_class_11 #education #New_first_year_chemistry This is brand new series for class 11 chemistry students, 2025. New book is going to complete, This lecture covers some important definitions such as standard enthalpy of reaction, enthalpy of combustion, enthalpy of formation, enthalpy of atomization, enthalpy of neutralization, and standard enthalpy of electron affinity with quick checks 6.1 and 6.2 from chapter 6 ( Chemical energetics). Join now and Subscribe for latest lectures in High Achievers Chemistry Batch by Sir Umair Khan. 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 5 https://umairkhanacademy.com/class-11... #11th_chemistry_new_book_2025 #chemicalenergetics #BondEnergy #highachieverschemistry #umairkhanacademy #1styearchemistry2025 #chemistry2025 #fscchemistry2025 #sirumairkhan Related Searches: Define thermodynamics, the science of relationships between heat and energy forms. Define thermochemistry, concerned with heat absorbed or evolved in changes. Explain the First Law of Thermodynamics, energy conservation principle applied to enthalpy changes. Define enthalpy, the sum of all potential and kinetic energies of a system. Define enthalpy change, the net energy evolved or absorbed as heat. Define exothermic process, where heat evolved, and Delta H is negative. Define endothermic process, where heat is absorbed, and Delta H is positive. Interpret a reaction pathway diagram, in terms of enthalpy change and activation energy. Define activation energy, minimum energy needed for reaction initiation. Define standard conditions, 25 C temperature and 1atm pressure. Define standard state of an element, its most stable form under 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. Calculate the entropy change for a reaction, given standard entropies of reactants and products. Define Gibbs free energy, determining reaction feasibility or spontaneity readily. Explain the relationship Gibbs free energy, Delta G equals Delta H minus T Delta S. Apply the concept of Gibbs free energy, to predict reaction spontaneity accurately.