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Chemistry 1A > Week Eight > Flashcards

Week Eight Flashcards

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1
Q

Entropy

A

spontaneous processes tend to proceed from states of low probability to states of higher probabilty
spontaneous processes tend to disperse energy

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2
Q

Delta S

A

Sproducts - Sreactants

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3
Q

Spontaneous event

A

accompanied by an increase in entropy of the system

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4
Q

Entropy change of a process

A

change in heat/ temp

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5
Q

Factors that affect entropy

A

volume
temperature
physical state
number of particles

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6
Q

Volume

A

possible to predict whether delta S is positive or negative

entropy increases with increasing volume for gases

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7
Q

Temperature

A

higher the temp, higher the entropy

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8
Q

Physical state

A

solid –> liquid –> gas

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9
Q

Number of particles

A

when all other things are equal, reactions that increase the number of particles in the system tend to have positive entropy change

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10
Q

Second law of thermodynamics

A

whenever spontaneous event occurs in universe, total entropy of the universe increases

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11
Q

Entropy change of universe equation

A

= entropy change of system + entropy change of surroundings

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12
Q

Entropy change for surroundings

A

equal to heat transferred to surroundings from system / Temp

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13
Q

Change in entropy surroundings

A

change in heat surroundings/ temperature

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14
Q

Change of entropy system

A
  • change in heat surroundings/ temperature or - change enthalpy system/ temperature
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15
Q

Total entropy change

A

change of entropy system - change in enthalpy system/ temperature

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16
Q

Gibbs free energy

A

H - T x s

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17
Q

Gibbs free energy change

A

delta H - T x delta S

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18
Q

Third Law of thermodynamics

A

at absolute zero, the entropy of a perfectly ordered pure crystalline substance is zero
provides point at which absolute entropy is known

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19
Q

Standard entropy

A

entropy of 1 mol of a substance determined at standard conditions at a temp of 298K

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20
Q

Entropy positive - enthalpy positive

A

spontaneous at high temps, non spontaneous at low temps

21
Q

Entropy positive - enthalpy negative

A

spontaneous at all temps

22
Q

Entropy negative - enthalpy positive

A

non spontaneous at all temps

23
Q

Entropy negative - enthalpy negative

A

non spontaneous at high temps, spontaneous at low temps

24
Q

Standard gibbs free energy change

A

when change in gibbs is determined at standard pressure, this is called standard free energy change

25
Q

Standard free energy change

A

change in Heat at standard - temp x change in entropy at standard

26
Q

Maximum conversion of chemical energy into work

A

can only occur if a process is thermodynamically reversible Requires the system to operate at equilibrium constantly

27
Q

Equilibrium

A

when a reactions forward and reverse reactions are occuring at same speed
no net change in overall composition

28
Q

Kc

A

equilbrium constant

29
Q

Kc equation

A 
    {A}^a {B}^b
30
Q

temperature effect on Kc

A

dependent on temp so temp is always specified

31
Q

Qc

A

reaction quotient

same as equilbirum equation but not all values are at equilbrium

32
Q

Kc rules

A

can only have one positive value at specific temp

33
Q

QC rules

A

can have multiple positive values

34
Q

Qc = Kc

A

at equilibrium

35
Q

Qc> Kc

A

when system reacts to use up all products and generate more reactants

36
Q

Qc< Kc

A

when system reacts to use up all reactants and generates more products

37
Q

Kp

A

uses partial pressure to specify the quantity of the two gases

38
Q

Kp equation

A

Kp = kc x (RxT / standard pressure)^ delta n gas

39
Q

number of moles

A

n/1 mol

40
Q

Delta n gas

A

(number of moles of gaseous products) - number of moles of gaseous reactants)

41
Q

Kc’

A

1/ Kc

when reaction is flipped

42
Q

Kc< 1

A

more reactant

43
Q

Kc = 1

A

same amounts of products and reactants

44
Q

Kc > 1

A

more product

45
Q

Homogeneous

A

all reactants and products are in same phase

46
Q

Heterogeneous

A

more than one phase

47
Q

Kc - structure of molecules

A

cant include the concentration of pure solids or pure liquids

48
Q

Pure liquids and solids at constant temp

A

ratio of amount of substance to volume of substance is constant

Chemistry 1A (12 decks)

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