Please enable JavaScript.
Coggle requires JavaScript to display documents.
Energetics - Coggle Diagram
Energetics
Enthalpy
Enthalpy Definitions
ΔH f Ꝋ = The enthalpy change when one mole of compound is formed from elements in their standard state
ΔH c Ꝋ = The enthalpy change when one mole of substance is burnt with excess oxygen in standard state
ΔH r Ꝋ = The enthalpy change when the reactants in the stoichiometric equation react to give the products under standard conditions
ΔH Neut Ꝋ = The enthalpy change when one mole of water is formed from reacting an acid with an alkali in standard state
-
Hess's Law, Born Haber Cycle
Hess's Law
The total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place as long as the initial and final conditions are the same
Born Haber Cycle
Definitions
Lattice enthalpy = the energy change when one mole of an ionic compound is separated into its component gaseous ions
First ionisation energy = the standard enthalpy change when one mole of gaseous atoms is converted into one mole of gaseous ions each with a single positive charge
Atomization = the enthalpy change when one mole of gaseous atoms from the element in its standard state under standard conditions
Electron Affinity = the standard enthalpy change when one mole of gaseous atoms is converted to one mole of gaseous ions, each with a single negative charge
-
-