q = mc∆T
∆H = -mc∆T
q = enthalpy change of water m = mass of water
c = specific heat capacity of water
∆T = change in temperature of water
∆H = enthalpy change of the reactants
Definitions I need to learn
Enthalpy change of formation
Enthalpy change of atomisation of an element
Enthalpy change of atomisation of a compound
Enthalpy change of neutralisation
Ionisation energy Electron affinity
Enthalpy change of hydration
Enthalpy change of solution
Standard Lattice Enthalpy: the enthalpy change when 1mole of a solid ionic compound is formed from its gaseous ions under standard conditions. It's a measure of ionic bond strength.
Higher ion charge = more energy released forming a lattice, so the enthalpy will be more negative.
Smaller ionic radii = more exothermic lattice enthalpy. Smaller ions pack closer together, meaning a stronger attraction because of the high charge density.
Born-Haber cycles are used to find out what the enthalpy change would be if you took a less direct route....
1) Start with the Enthalpy change of Formation at the bottom
2) Put the enthalpies of atomisation and ionisation above
3) The electron affinity goes on the top right
Sum of clockwise arrows = Sum of anti-clockwise arrows