Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Physical Chemistry Year 2 > 3.1.8 thermodynamics > Flashcards

3.1.8 thermodynamics Flashcards

1
Q

enthalpy change

A

heat energy change at constant pressure

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

exothermic (-ve) / endothermic (+ve)

A

either

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

enthalpy of formation

A

enthalpy change when one mole of a substance is formed from its constituent elements with all substances in their standard states

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

equation for formation of water

A

H2(g) + 1/2 O2 (g) -> H20 (l)

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

exothermic (-ve) / endothermic (+ve)

A

mostly exothermic

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

enthalpy of combustion

A

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

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

equation for methane

A

CH4 (g) + 2O2 (g) -> CO2 (g) + 2H20 (l)

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

equation for methane

A

CH4 (g) + 2O2 (g) -> CO2 (g) + 2H20 (l)

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

exothermic (-ve) / endothermic (+ve)

A

exothermic

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

enthalpy of neutralisation

A

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

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

exothermic (-ve) / endothermic (+ve)

A

exothermic

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

enthalpy of atomisation

A

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

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

exothermic (-ve) / endothermic (+ve)

A

endothermic

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

first ionisation energy

A

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

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

equation for magnesium

A

Mg (g) -> Mg^+ (g) + e-

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

exothermic (-ve) / endothermic (+ve)

A

endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

second 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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

equation for magnesium

A

Mg+(g) -> Mg^2+ (g) + e-

19
Q

exothermic (-ve) / endothermic (+ve)

A

endothermic

20
Q

first 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

21
Q

equation for oxygen

A

O(g) + e- -> O^- (g)

22
Q

exothermic (-ve) / endothermic (+ve)

A

exothermic

23
Q

second electron affinity

A

enthalpy change when each ion in one mole of gaseous 1- ions gains one electron to form one mole of gaseous 2- ions

24
Q

equation for oxygen

A

O- (g) + e- -> O^2- (g)

25
Q

exothermic (-ve) / endothermic (+ve)

A

endothermic (as adding -ve electron to -be ion)

26
Q

lattice enthalpy of formation

A

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

27
Q

equation for sodium chloride

A

Na+ (g) + Cl- (g) -> NaCl (s)

28
Q

exothermic (-ve) / endothermic (+ve)

A

exothermic

29
Q

lattice enthalpy of dissociation

A

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

30
Q

exothermic (-ve) / endothermic (+ve)

A

endothermic

31
Q

enthalpy of hydration

A

enthalpy change when one mole of gaseous ions become hydrated (dissolved in water)

32
Q

equation for sodium

A

Na+ (g) + aq -> Na+ (aq)

33
Q

exothermic (-ve) / endothermic (+ve)

A

exothermic

34
Q

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 don’t interact with each other

35
Q

equation for sodium chloride

A

NaCl (aq) + aq -> Na+ (aq) + Cl- (aq)

36
Q

exothermic (-ve) / endothermic (+ve)

37
Q

bond dissociation enthalpy

A

enthalpy change when one mole of covalent bonds is broken in the gaseous state

38
Q

exothermic (-ve) / endothermic (+ve)

A

endothermic

39
Q

mean bond enthalpy

A

enthalpy change when one mole of gaseous molecules each breaks a covalent bond to form two free radicals, averaged over a range of compounds

40
Q

exothermic (-ve) / endothermic (+ve)

41
Q

enthalpy of vaporisation

A

enthalpy change when one mole of a liquid is turned into a gas

42
Q

exothermic (-ve) / endothermic (+ve)

A

endothermic

43
Q

enthalpy of fusion

A

enthalpy change when one mole of a solid is turned into a liquid

44
Q

exothermic (-ve) / endothermic (+ve)

A

endothermic

Physical Chemistry Year 2 (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions