Thermodynamics Flashcards

1
Q

Define enthalpy change of formation

A

Enthalpy change when one mole of a substance is formed from its constituent elements with all substance in their substances
-exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Define enthalpy change of combustion

A

Enthalpy change when one mole of a substance undergoes complete combustion in oxygen with all substances in standard states
-exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Define enthalpy of neutralisation

A

enthalpy change when 1 mole of water is formed in a reaction between an acid and alkali under standards conditions
-exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Define 1st ionisation enthalpy

A

Enthalpy change when each atom in one mole of gaseous atoms loses one electron to form one mole of gaseous 1+ ions
-endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define 2nd ionisation energy

A

Enthalpy change when each ion in one mole of gaseous 1+ ions loses one electron to form one mole of gaseous 2+ ions
-endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Define 1st electron affinity

A

Enthalpy change when each atom in one mole of gaseous atoms gains one electron to form one mole of gaseous 1-ions
exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Define 2nd electron affinity

A

Enthalpy change when each ion in one mole of gaseous ions gains one electron to form one mole of gaseous 2- ions
endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Define enthalpy change of atomisation

A

Enthalpy change when one mole of gaseous atoms is produced from an element in its standard state
-endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Define hydration enthalpy

A

Enthalpy change when one mole of gaseous ions become hydrated(dissolved in water)
-exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Define enthalpy of solution

A

Enthalpy change when one mole of an ionic solid dissolves in an amount of water large enough so that the dissolved ions are well separated and do not interact with each other
exothermic/endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Define bond dissociation enthalpy

A

Enthalpy change when one mole of covalent bond is broken in the gaseous state
-endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Define lattice enthalpy of formation

A

Enthalpy change when one mole of a solid ionic compound is formed from into its constituent ions in the gas phase
exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Define lattice enthalpy of disassociation

A

Enthalpy change when one mole of a solid ionic compound is broken up into its constituent ions is the gas phase
endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Enthalpy change of vaporisation

A

Enthalpy change when one mole of a liquid is turned into a gas
endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Define enthalpy of fusion

A

Enthalpy change when one mole of a solid is turned into a liquid
endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Define bond enthalpy

A

Mean value across a range of compounds containing that bond

17
Q

Define enthalpy change

A

The heat change measured under conditions of constant pressure

18
Q

Define standard conditions

A

100kPa and stated temp. (eg 298K)