Energetics II Flashcards
what is lattice energy?
the energy change when one mole of an ionic solid is formed from its gaseous ions under standard conditions (298K 100kPa)
what is enthalpy change of atomisation, ΔatH?
Enthalpy change when 1 mole of gaseous atoms is formed from the elements in its standard states. Always endothermic.
what is electron affinity?
the energy change when each atom in one mole of atoms in the gaseous state gains an electron to form a -1 ion
what is lattice energy a measure of?
ionic bond strength
what is ‘enthalpy change of solution, ΔsolH?
enthalpy change when one mole of solute dissolves in water
what is ‘enthalpy
change of hydration, ΔhydH’?
enthalpy change when one mole of gaseous ions dissolves in water
if lattice energy is more negative what does this imply?
the ionic bonding of the compound is strong
what is the unit for entropy?
K-1 mol-1
what is the formula for entropy change in the surroundings?
∆ S surroundings = -∆sol H/T
what is the formula for ΔStotal?
ΔS total = ΔS system + ΔS surroundings
what is the formula for charge density?
charge/volume
what is the formula or free energy?
ΔG = ΔH – TΔS
ΔG is the change in free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy
what must the value of ΔG be in order for a reaction to be feasible?
zero or negative (the more negative the more feasible)
if ΔH is negative and ΔS is positive will the reaction be feasible?
Yes because ΔG will be negative
if ΔH is positive and ΔS is negative will the reaction be feasible?
No because ΔG will be positive