Energetics Flashcards
Standard enthalpy change of reaction
The enthalpy change when molar quantities of reactants stated in the chemical equation react to form products under Standard condition.
Standard Condition
298K, 1 bar Pressure, solutions at 1moldm-3
Bond energy
The enthalpy change to break 1 mole of covalent bond between 2 gaseous atom.
Calculation of Standard enthalpy change of reaction
1) BE(Rxt) - BE(Pdt)
2) Hc(Rxt) - Hc(Pdt)
3) Hf(Pdt) - Hf(Rxt)
Standard Enthalpy change of Atomisation for elements
Enthalpy change in forming 1 mole of gaseous atom from its element in their standard state at standard condition
Standard Enthalpy change of Atomisation of compound
The enthalpy change in forming gaseous atoms from 1 mole of substance at standard condition.
Standard enthalpy change of Combustion
The enthalpy change to completely burn 1 mole of substance in excess oxygen at standard condition
Standard enthalpy change of Formation
Enthalpy change in forming 1 mole of compound from their constituent elements in their standard state at standard condition.
Standard enthalpy change of Neutralisation
The enthalpy change when an acid react with base to form 1 mole of water in dilute aqueous solution at standard condition.
Hess’ Law
The enthalpy change of a reaction is the same regardless of path taken, given initial state of reactant and final state of product are the same
Lattice Energy
The enthalpy change to form 1 mole of solid ionic compound from its constituent gaseous ions.
First Ionisation Energy
Energy required to remove 1 mole of electrons from 1 mole of gaseous atom to form 1 mole of singly charged gaseous cations.
First Electron Affinity
The enthalpy change when 1 mole of electrons is gained by 1 mole of gaseous atoms to form 1 mole of singly charged gaseous anions.
Standard enthalpy change of Hydration
The enthalpy change when 1 mole of the gaseous ions dissolve in a large amount of water to form 1 mole of aqueous ion under Standard Condition
Standard Enthalpy change of Solution
The enthalpy change when 1 mole of substance is completely dissolved in a large excess of solvent to form an infinitely dilute solution at Standard condition.
Equation for H(soln)
H(soln) = H(Hyd)-LE
Entropy
A quantity which measure degree of disorder of a system
Factors affecting Entropy
1) Change in Temp
2) Change in States
3) Change in number of particles
4) Mixing of Particles (Gas and Solid)
Standard Gibbs free energy change of reaction
The maximum amount of energy that is available to do work under Standard Condition
Units= kJ mol-1
Equation of G
Change in G = Change in Enthalpy energy - T(Change in Entropy)