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CHEM191 > Module 1 and 2 > Flashcards

Module 1 and 2 Flashcards

1
Q

K > Q which reaction is favoured

A

Forward

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2
Q

K < Q which reaction is favoured

A

Backward

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3
Q

Will a precipitate form if Q > K

A

Yes

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4
Q

Will a precipitate form if Q < K

A

No

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5
Q

The stronger the acid or base, the _____ the conjugate

A

Weaker

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6
Q

Ligands act as

A

Lewis bases

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7
Q

Acid base reactions involve the exchange of

A

1 proton

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8
Q

Redox reactions involve the exchange of

A

Electrons

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9
Q

“X is titrated with Y” (where are these solutions located)

A

X in flask (unknown concentration), Y in burette (known concentration)

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10
Q

Ratio of buffer made with weak acid or base and conjugate

A

1:1

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11
Q

Ratio of buffer made with weak acid/base and strong acid/base

A

2:1

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12
Q

Ionisation status depends on

A

pH of solution and pKa of functional group

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13
Q

Percent protonated when >1 unit below pKa

A

90%

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14
Q

Percent deprotonated when >1 unit above pKa

A

90%

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15
Q

Amino acid pKa below which all are protonated

A

2.5

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16
Q

Amino acid pKa above which all are deprotonated

A

9.5

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17
Q

𝚫fH

A

change in enthalpy for the formation of 1 mole of a compound from its constituent elements in their standard states (already in standard states= 0)

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18
Q

𝚫vapH

A

change in enthalpy for one mole of a substance changing from a liquid to a gas

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19
Q

𝚫fusH

A

change in enthalpy for one mole of a substance changing from a solid to a liquid

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20
Q

𝚫comH

A

change in enthalpy for the combustion of one mole of a substance in oxygen (products CO2, H2O)

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21
Q

Negative change in enthalpy

A

Exothermic

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22
Q

Positive change in enthalpy

A

Endothermic

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23
Q

Spontaneous meaning

A

Once started continues without help, not necessarily to completion

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24
Q

Standard entropy conditions

A

1molL^-1, 1 bar pressure, no value for temperature

25
Q

Positive Gibbs energy

A

Non spontaneous under standard conditions

26
Q

Negative Gibbs energy

A

Spontaneous under standard conditions

27
Q

Gibbs energy = 0

A

Equilibrium

28
Q

What does the magnitude of G tell us

A

How far a reaction will go to completion (no absolute value of G)

29
Q

𝚫fG for a pure element

30
Q

Units for enthalpy

31
Q

Units for entropy

A

JK^-1mol^-1

32
Q

Positive enthalpy and entropy

A

Spontaneous at high temperatures

33
Q

Negative entropy, negative enthalpy

A

Spontaneous at low temperatures

34
Q

Positive entropy, negative enthalpy

A

Spontaneous at all temperatures

35
Q

Negative entropy, positive enthalpy

A

Non spontaneous at all temperatures

36
Q

Units of k 0th order

A

molL^-1s^-1

37
Q

Units of k 1st order

38
Q

Units of k 2nd order

A

Lmol^-1s^-1

39
Q

Units of k 3rd order

A

L^2mol^-2s^-1

40
Q

What is a pseudo first order reaction

A

[B]&raquo_space; [A], when [B] changes [A] doesn’t change much

41
Q

Unit for rate

A

molL^-1s^-1

42
Q

What is Ea

A

Energy difference between reactant and highest energy transition state

43
Q

Straight line Arrhenius equation rearrangement

A

lnk = -Ea/R 1/T + lnA

44
Q

When can you use the integrated rate law

A

Only for first order reactions

45
Q

The rate doubles for every ___ increase in temperature

46
Q

E standard will always be _____ for a spontaneous reaction

47
Q

The smaller the Ka or Kb, the _____ the acid or base

48
Q

The larger the pKa or pKb, the _____ the acid or base

49
Q

The larger the Ka or Kb, the _____ the acid or base

50
Q

The smaller the pKa or pKb, the _____ the acid or base

51
Q

Ligand definition

A

Molecule or ion in which one or more donor atoms have a lone pair of electrons (biologically important donor atoms: N, O, P, S) (an ion or molecule attached to a metal atom by coordinate bonding.)

52
Q

Ligands act as

A

Lewis bases (donate electrons to transitional metal ion)

53
Q

When water is the ligand, resulting complex can act as

54
Q

Ligand complex becomes more acidic as

A

Charge on cation increases

55
Q

What doesn’t appear in Kc expressions

A

Pure solids AND liquids

56
Q

The _____ the acid or base, the ______ the conjugate

A

Stronger, weaker

57
Q

Straight line axes for linear first order reaction

A

ln[X] vs t

58
Q

Arrhenius equation

A

K = Ae^-Ea/RT

CHEM191 (1 decks)

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