A2 Aqa Chemistry : Thermodynamics

Front 1

What are standard conditions?

Back 1

100kPa and 298K

Front 2

Define Lattice formation enthalpy

Back 2

the enthalpy change when one mole of a solid ionic compound is formed from its gaseous ions under standard conditions

Front 3

Define Lattice dissociation enthalpy

Back 3

the enthalpy change when one mole of a solid ionic compound is completely disassociated into its gaseous ions under standard conditions

Front 4

Define enthalpy change of formation

Back 4

the enthalpy change when one mole of a compound is formed from its elements in standard states and under standard conditions

Front 5

define enthalpy change of combustion

Back 5

the enthalpy change change when one mole of a compound is completely combusted under standard conditions

Front 6

define bond dissociation enthalpy

Back 6

the enthalpy change when all the bonds of the same type in one mole of gaseous molecules are broken

Front 7

define enthalpy change of atomisation (element)

Back 7

the enthalpy change when one mole of of gaseous atoms is formed from an element in its standard state

Front 8

define enthalpy change of atomisation (compound)

Back 8

the enthalpy change when one mole of a compound in its standard state is converted into gaseous atoms

Front 9

define first ionisation energy

Back 9

the enthalpy change when one mole of gaseous +1 ions is formed from one mole of gaseous atoms

Front 10

define second ionisation energy

Back 10

the enthalpy change when one mole of gaseous +2 ions is formed from one mole of gaseous +1 ions

Front 11

define first electron affinity

Back 11

the enthalpy change when one mole of gaseous -1 ions is made from one mole of gaseous atoms

Front 12

define second electron affinity

Back 12

the enthalpy change when one mole of gaseous -2 ions is made from one mole of gaseous -1 ions

Front 13

define enthalpy change of hydration

Back 13

the enthalpy change when one mole of aqueous ions is formed from gaseous ions

Front 14

define enthalpy change of solution

Back 14

the enthalpy change when one mole of solute is dissolved in sufficient solvent that no further enthalpy change occurs on further dilution

Front 15

what does Hess's law state ?

Back 15

that the total enthalpy of a reaction is always the same no matter which route is taken