Energetics equations Flashcards
Spontaneity
The ability of a reaction ONCE INITIATED to progress in a given direction without any extra input of energy
Gibbs Free Energy
the measure of the maximum amount of net useful work that can be obtained from a reaction
Entropy
The number of ways available energy can be distributed amongst particles.
Enthalpy change of solution
Enthalpy change when 1 mole of solute is dissolved in an infinite volume of water, under standard conditions
Enthalpies of hydration
The energy released when 1 mole of gaseous ions is dissolved to form an infinitely dilute solution of 1 mole of aqueous ions.
Lattice enthalpy
The energy needed to convert 1 mole of a solid ionic compound into its gaseous ions.
Enthalpy of formation
Enthalpy change when 1 mole of a substance is formed from its elements in their standard states.
Bond enthalpy
Enthalpy change when 1 mole of a covalent bond is broken to form atoms, all species in the gaseous phase
Average bond enthalpy
The average amount of energy needed to break 1 mole of covalent bonds between 2 atoms, to form atoms, all species in the gaseous phase. Bond enthalpies vary across different compounds so it is the average of the bond enthalpies across multiple similar compounds
First/second ionisation enthalpy change
Enthalpy change accompanying the removal of 1 mole of electrons/seconds electrons from 1 mole of atoms/singly + charged ions in the gaseous phase
First/second electron affinity
Enthalpy change accompanying the additions of 1 mole of electrons to 1 mole of atoms/singly charged negative ions in the gaseous phase
Enthalpy change of atomisation
Enthalpy change accompanying the formation of 1 mole of gaseous atoms from the element in its standard state
