Thermodynamics Flashcards
Define lattice formation of enthalpy
Enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions
Define lattice dissociation enthalpy
Enthalpy change when 1 mole of a solid ionic compound is completely dissociated into its gaseous ions
What does a big difference in theoretical and experimental enthalpy change tell you?
Shows ionic bonds are strongly polarised with a large degree of covalency
Enthalpy change of formation
Enthalpy change when 1 mole of a compound is formed from its elements in their standard states
Bond dissociation enthalpy
Enthalpy change when all the bonds of the same type in 1 mole of gaseous molecules are broken
Enthalpy change of atomisation of an element
Enthalpy change when 1 mole of gaseous atoms is formed from an element in its standard state
Enthalpy change of atomisation of a compound
Enthalpy change when 1 mole of a compound in its standard state is converted to gaseous atoms
1st ionisation energy
Enthalpy change when 1 mole of gaseous 1+ ions is formed from 1 mole of gaseous atoms
2nd ionisation energy
Enthalpy change when 1 mole of gaseous 2+ ions is formed from 1 mole of gaseous 1+ ions
1st electron affinity
Enthalpy change when 1 mole of gaseous 1- ions is formed from 1 mole of gaseous atoms
2nd electron affinity
Enthalpy change when 1 mole of gaseous 2- ions is made from 1 mole of gaseous 1- ions
Enthalpy change of hydration
Enthalpy change when 1 mole of aqueous ions is formed from gaseous ions
Enthalpy change of solution
Enthalpy change when 1 mole of an ionic substance dissolves enough solvent to form an infinitely dilute solution
Define entropy
The measure of the disorder of a system
Equation for S, entropy change
Unit?
What does a positive value for Ssystem tell you?
Ssystem = Sprod - Sreac
JK-1mol-1
Right side of the reaction is favoured
What happens to entropy of temperature decreases?
If moles increase?
Entropy decreases
Entropy increase
Define free energy change
Energy available for work, predicting whether reaction is feasible
Equation for free energy change, G
Unit?
G = H - TS
H = enthalpy change, T = temp (K), S = entropy
What value of G is required for a reaction to be feasible?
G = 0 or less
Equation for total enthalpy change of a reaction
H = Hprod - Hreac (AS equation)
How do u you find the temperature at which a reaction becomes feasible?
Make G = 0 and rearrange for T in the equation, G = H -TS