Thermodynamics Flashcards
Define Lattice dissociation Enthalpy
- energy require to break apart and ionic lattice
- into its constituent ions in their gaseous state
- under standard conditions
Define Lattice formation enthalpy
- energy required to form an ionic lattice
- from its constituent ions in gaseous state
- under standard conditions
Define atomisation enthalpy
- energy required to form 1 mole
- of gaseous atoms
- under standard conditions
Define Enthalpy of electron affinity
- energy required when 1 mole of electrons
- are added to 1 mole of gaseous atoms
- under standard conditions
Define enthalpy of solution
- energy change when 1 mole of an ionic solid
- is dissolved in water to infinite dilution
- under standard conditions
Define enthalpy of hydration
- energy change when 1 mole of gaseous atoms
- are dissolved in water to form 1 mole of aqueous ions
- under standard conditions
What are two assumptions you mae in the perfect ionic model
- All the ions are perfectcly spherical
- All ions have no covalent character
What is covalent character
- when two joined ions have varying sizes or charges, meaning the distribution of charge is not even
What is entropy
A measue of disorder
What happens to entropy as temp increases
As temp increases, entropy increases because particles gain more energy, and move further apart, and become less ordered
What state has the highest entropy
gas
What do you measure entropy in
J K –1 mol –1.
What is the equation for total entropy
entropy total = (entropy products) - (entropy reactants)
Considering all things tend towards a state of disorder, what kind if entropy do spontaneous reactions have
positive ( more disordered)
What is gibbs free energy equation
G= enthalpy change - temp(entropy change)
