Thermochemistry-Key Point

Key Concepts in Thermochemistry

1. Thermochemistry: The study of heat change during a chemical reaction.
2. Endothermic Reactions: Reactions accompanied by the absorption of heat.
3. Enthalpy of Solution: Heat change when one mole of a substance dissolves in a solvent at a given temperature.
4. Enthalpy: Total heat content of a system (H = E + PV).
5. Exothermic Reactions: Reactions accompanied by the release of heat.
6. State Function: A property that depends only on the current state of the system, not on the path taken to reach that state.
7. Surroundings: Everything outside the system under study.
8. System: The part of the universe under study (e.g., reactants/products).
9. First Law of Thermodynamics: Energy can neither be created nor destroyed but can change form.
10. Irreversible Reaction: A reaction where products do not revert to original reactants under the same conditions.
11. Non-spontaneous Process: A process that does not occur naturally and requires external energy.
12. Reversible Reaction: A reaction where products can reform original reactants.
13. Spontaneous Process: A natural process that occurs without external help and leads to equilibrium.
14. Heat Capacity: Heat required to raise the temperature of a substance by 1K.
15. Bond Dissociation Energy: Energy required to break one mole of a specific bond in gaseous molecules.
16. Standard Enthalpy of Atomization: Enthalpy change when one mole of gaseous atoms is formed from its element in standard conditions.
17. Standard Enthalpy of Formation: Enthalpy change when one mole of a compound forms from its elements in standard conditions.
18. Standard Enthalpy of Neutralization: Heat evolved when one mole of H⁺ reacts with one mole of OH^- to form water under standard conditions.
19. Hess's Law: Total enthalpy change is the same regardless of the reaction path, provided initial and final conditions are constant.
20. Calorimeter: A device used to measure heat flow in a chemical reaction or process.

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