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ATARChemU1T3Flash

QuestionAnswer
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 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.
Empirical formula Formula of a compound showing the simplest whole number ratio of atoms of different elements in the compound
Formula unit Term for ionic compounds (smallest whole number ratio of the compound)
Molecular formula Formula of a compound showing the actual number of atoms of different elements covalently bonded in a molecule
Entropy (S) The degree of randomness
Created by: andrewweng0406
 

 



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