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IB Chem 5 SL

Temperature the average kinetic energy of molecules (K).
Heat the amount of energy exchanged due to a temperature difference between two substances (J).
Enthalpy (H) the amount of energy or heat content of a substance.
Standard enthalpy change of reaction (ΔH⁰) the difference between the enthalpy of the products and the enthalpy of the reactants at 298K and 1.00 x 10E5Pa.
Change in enthalpy (ΔH) enthalpy of products less reactants. It is the heat energy change per mole.
exothermic reactions the temperature of the surroundings increases and ΔH is negative
endothermic reactions the temperature of the surroundings decreases and ΔH is positive
Hess’s Law In a chemical reaction the total change in chemical potential energy (enthalpy change) must be equal to the energy lost or gained by the reaction system.
Standard enthalpy change of formation (ΔH⁰f) the enthalpy change that results when one mole of a compound is formed from its elements at 298K and 1.00 x 10E5Pa.
Standard enthalpy change of combustion (ΔH⁰C) the enthalpy change that results when one mole of a compound reacts with oxygen at 298K and 1.00 x 10E5Pa
Average bond enthalpy the amount of energy required to break one mole of bonds in the gaseous state averaged across a range of compounds containing that bond.
Created by: andrewweng0406



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