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Chemistry > Module 5 > Flashcards

Module 5 Flashcards

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1
Q

Conc. time graphs?

A

Zero - \
1st - curve down
2nd - large surge down

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2
Q

Rate conc. graph?

A 
Zero =  — 
1st = / 
2nd = curve up
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3
Q

Rate determining step

A

The slowest step within the sequence

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4
Q

Arrenhius equation?

A

K = A e-Ea/RT

Log
LnK = -Ea/RT + LnA
Y = mx + c

Gradient = -Ea/R
Y axis intercept = lnA

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5
Q

Mole fraction?

A

No of moles of A / no of moles in gas mixture

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6
Q

Partial pressure?

A

Mole fraction of A X total pressure

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7
Q

Weak acid calc?

A

Ka

HA <=> H+ + A-

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8
Q

Strong bad/ strong acid?

A

Kw
Kw = [H+][OH-]
1 x 10-14

Weak base = POH = -log(OH-)
pH = 14 - POH

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9
Q

Buffer

A

System that minimises pH changes when small amounts of an acid or base are added

Weak acid and conjugate base

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10
Q

Titration curves?

A

Neutralisation

Equivalence point - volume of one solution that exactly reacts with the volume of the other

End point - indicator contains equal concentrations of HA and A-, colour between the two

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11
Q

Lattice enthalpy?

A

The enthalpy change that accompanied the formation of one moles of an ionic compound from its gaseous ions

K+ + cl- —> kcl (s)

Exothermic always negative

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12
Q

Enthalpy change of formation

A

EC that takes place when one mole of a compound is formed from its elements

Na (g) + 1/2Cl2 (g) —> Nacl (s)

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13
Q

Enthalpy change of atomisation?

A

EC that takes place for the formation of one mole of a gaseous atom from the element

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14
Q

First ionisation energy

A

The enthalpy change required to remove one electron from each atom of one mole of gaseous atoms to form one mole of gaseous +1 ions

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15
Q

First electron affinity

A

Energy change that takes place when one electron is added to an atom in one mole of gaseous atoms to form one mole of gaseous -1 ions

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16
Q

Enthalpy change of solution

A

Enthalpy change that take solace when one mole of a solute dissolves in a solvent

17
Q

Enthalpy change of hydration

A

Enthalpy change that accompanies the dissolving of gaseous ions in water to form aqueous ions

18
Q

Factors affecting lattice enthalpy

A

Ionice size - increase, attraction between ions decreases, lattice enthalpy less negative, MP decrease

Ionic charge - increases, attraction increase, lattice enthalpy more negative

19
Q

Factors affecting hydration enthalpy

A

Ionic size - increase, attraction between water molecules and ions decreases, hydration energy less negative

Ionic charge - increase, attraction with water molecules increase, more negative

20
Q

Entropy?

A

🔼s
The greater the entropy the greater the dispersal of energy hence the greater the disorder

At 0K no energy entropy 0
Always Positive entropy

21
Q

Standard entropy?

A

Entropy of one mole of a substance, standard conditions

22
Q

Gibbs free energy

A

🔼G = 🔼H - t🔼S

🔼G < 0 to be feasible

23
Q

Primary fuel cell

A

Non rechargeable
Electrical energy produced by oxidation and reduction of electrodes
Reactions cannot be reversed, chemicals used up and voltage will fall.
Generally alkaline based

24
Q

Secondary fuel cell?

A

Rechargeable

Reversed during recharging, chemicals regenerated

25
Q

Fuel cells?

A

Use energy from the reaction of a fuel with oxygen to create a voltage

26
Q

Transition elements

A

Dblock elements that form at least one ion egg a partially filled d-orbital

Form compounds with different oxidation states
Form coloured compounds
Can act as catalysts

27
Q

Complex ions

A

Formed when one or more negatively charged ions bond to central metal ions (Ligands)

Ligand - molecule or ion that donates pair of e- to central metal ion to form coordinate bond

28
Q

Ligand substitution

Copper and ammonia

A

Cooper ions and ammonia

[Cu(H2O)6]2+ pale blue
add ammonia

First see pale blue ppt Cu(OH)2
Then ppt dissolves in excess ammonia create dark blue solution [Cu(NH2)4(H2O)2]2+

29
Q

Ligand substitution

Copper and chloride

A

[Cu(H2O)6]2+ pale blue
Add 4Cl-

[CuCl4]2- yellow solution

30
Q

Ligand substitution

Chromium ions

A

Chromium sulphate dissolved in water

[Cr(H2O)5SO4]+ green solution

31
Q

Precipitation reaction?

A

Two aqueous solutions containing ions react together to form an insoluble ionic solid precipitate.

32
Q

Qualitative analysis

A 
Cu2+ blue —> blue ppt 
Fe2+ pale green —> green ppt
Fe3+ pale yellow —> orange/brown ppt 
Mn2+ pale pink —> pink/brown ppt 
Cr3+ violet —> grey/green ppt

Addition of OH-

Chemistry (3 decks)

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