Energetics

1. heat change in a chemical reaction is the same regardless of the number of stages in which the reaction is effected
5. amount of heat that is released or absorbed during the dissolving process (at constant pressure)
6. amount of energy required to completely separate one mole of the solid ionic compound into constituent gaseous ions
8. gradual thinning of Earth's ozone layer in the upper atmosphere caused by the release of chemical compounds containing gaseous chlorine or bromine from industry and other human activities
9. heat energy given out when one mole of a substance burns completely in oxygen
10. no reactants or products can escape, only heat can be exchanged freely
11. heat energy and matter can transfer freely between the surrounding and the containers
13. Chemical reactions that absorb (or use) energy overall
15. reaction can take place by more than one route from the same initial and final conditions then the total enthalpy change is the same for each route
17. cycle of enthalpy change of process that leads to the formation of a solid crystalline ionic compound from the elemental atoms in their standard state and of the enthalpy of formation of the solid compound such that the net enthalpy becomes zero

2. quantity of heat (J) absorbed per unit mass (kg) of the material when its temperature increases 1 K (or 1 °C)
3. standard reaction enthalpy for the formation of the compound from its elements (atoms or molecules) in their most stable reference states at the chosen temperature (298.15K) and at 1bar pressure
4. amount of energy released on dilution of one mole of gaseous ions
7. measure of a system's thermal energy per unit temperature that is unavailable for doing useful work
12. difference between total reactant and total product molar enthalpies
14. Chemical reactions that release energy
16. ratio of heat absorbed by a material to the temperature change
18. amount of energy stored in a bond between atoms in a molecule