mod 5 14.1 thermodynamics

14.1 Thermodynamics.

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  • Created by: HASNAAN
  • Created on: 14-06-09 15:13

Enthalpy change

Enthalpy change is the amount of heat energy taken in or given out during any physical or chemical change under constant pressure.

Standard Pressre - 100 KPa

Standard temprature - 298 K

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Standard enthalpy of formation

The enthalpy change when one mokle of a compound is formed from it's elements under standard conditions all reactants and products in there standard states.

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Ionisation enthalpy

standard molar enthalpy change for the removal of and electron from a species in the gas phase to form a positive ion and an electron, both also in the gas phase.

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Electron affinity

The standard molar enthalpy change when an electron is added to an isolated atom in the gas phase.

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Bond dissociation enthalpy

standard molar enthalpy change which accompanies the breaking of a covalent bond in a gaseous molecule to form two free radicals, also in the gas phase.

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Enthalpy of atomisation

is the standard enthalpy change which accompanies the formation of one mole of gaseous atoms.

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Lattice enthalpy

The standard molar enthalpy change which accompanies the separation of one mole of a solid ionic lattice into gaseous ions.

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Enthalpy of Hydration

Standard molar enthalpy change for the process...

X+/- (g)-----> X+/- (aq)


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enthalpy of solution

Standard enthalpy for the process in which one mole of an ionic solid dissolves in an amount of water large enough to ensure that the dissolved ions are well speprated and do not interact with one another.

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Gibbs free energy change.

^G must be negative or Zero for easible change.

^G = ^H - T^S

For a system at equllibrium ^G is 0

so...

^G = ^H - T^S goes to ^H - T^S

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