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Gen Chem > Lesson 6-10 > Flashcards

Lesson 6-10 Flashcards

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1
Q

The study of the rates of chemical reaction or how fast a reaction can occur is known as

A

Chemical Kinetics

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2
Q

Minimum amount of energy required to cause a reaction

A

Activation Energy

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3
Q

Molecules collide with sufficient energy and proper orientation, a reaction occurs. A product is formed.

A

Effective Collision

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4
Q

No product is formed

A

Ineffective Collision

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5
Q

Substances that help speed up the rate of chemical reactions

A

Catalysts

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6
Q

Process of speeding up a reaction using a catalyst

A

Catalysis

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7
Q

Reaction between a catalyst and a reactant

A

Catalytic Reaction

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8
Q

The catalyst and reactants are in the same physical state or phase

A

Homogenous Catalysis

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9
Q

The catalyst and reactants are in different phases

A

Heterogeneous Catalysis

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10
Q

Proteins that function as catalyst in all living systems. Natural Catalyst found in the body

A

Enzymes

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11
Q

True or False: Catalysts lower the energy required for the transition state of reaction to be reached

A

True

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12
Q

True or False: Catalysts affects the degree or the progress of the reaction

A

False

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13
Q

A measure of the disorder of a system

A

Entropy

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14
Q

Greater number of reactant molecules are more _______ at higher temperatures

A

Energetic

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15
Q

First Law of Thermodynamics

A

Conservation of Energy
Energy can change forms, but cannot be created nor destroyed

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16
Q

Second Law of Thermodynamics

A

In all the spontaneous processes, the entropy of the universe increases

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17
Q

Third Law of Thermodynamics

A

Entropy of a system approaches a constant as temperature approaches
absolute zero.

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18
Q

Entropy __________ in melting and evaporatoration

A

Increases

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19
Q

Entropy __________ in condensation and freezing

A

Decreases

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20
Q

Entropy Change Formula

A

△ S°rxn = S°(products) - S°(reactants)

△ S°sys = qrev/T

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21
Q

We expect an increase in entropy when

A

a gas is formed from the reactants

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22
Q

We expect a decrease in entropy when

A

a gaseous reactant is converted to a solid or liquid

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23
Q

There is a reduction in disorder during

A

synthesis reactions

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24
Q

There is an increase in disorder during

A

a decomposition reaction

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25
Q

The DEGREE OF DISORDERLINESS (ENTROPY) of a simple substance can generally be determined by

A

The number of arrangements that the molecules can have in the system

The number of type of molecules as well as the number of molecules.

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26
Q

Factors that combine to predict spontaneity

A

Energy Change, Temperature, Entropy Change

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27
Q

A reaction will ________ spontaneously move away from equilibrium and will always move spontaneously ________ equilibrium.

A

Never, Towards

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28
Q

A reaction that does occur under a given set of conditions is called

A

spontaneous reaction

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29
Q

If G is positive, then

A

the reaction is nonspontaneous

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30
Q

A reaction is at ________ state if the rate of the forward reaction equals the rate of the backward reaction.

A

equilibrium

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31
Q

mA + nB -> xC + yD

A

Qc = [(C^x) * (D^y)] / [(A^m) * (B^n)]

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32
Q

If Qc < Kc, then

A

The reaction proceeds on a forward direction

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33
Q

If Qc > Kc

A

Reaction proceeds on a reverse direction

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34
Q

If Qc = Kc

A

Reaction is at equilibrium

35
Q

reactions in which all reacting species are in the same phase.

A

homogeneous equilibrium

36
Q

aA + bB ⇌ cC + dD

A

Kc = [(C^c) * (D^d)] / [(A^a) * (B^b)]

37
Q

Le Chatelier’s Principle, states that

A

if an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position

38
Q

adding additional reactant to a system will shift the equilibrium to the

A

right, towards the side of the products

39
Q

Catalysts has ____________ on the equilibrium system

A

no effect

40
Q

Brensted-Lowry theory describes

A

acid-base interactions in terms of proton transfer between chemical species

41
Q

Bronsted acid is a

A

substance capable of donating a proton (H+ ions)

42
Q

Bronsted base is a

A

substance capable of accepting a proton (H+ ions)

43
Q

conjugate acid-base pair which can be defined as

A

an acid and its conjugate base or a base and its conjugate acid

44
Q

product formed when acid loses H+

A

Conjugate base

45
Q

product formed when base gains H+

A

Conjugate acid

46
Q

pH formula

A

pH = -log[H+]

47
Q

pH meaning

A

Power of Hydrogen, negative logarithm of the hydrogen ion concentration

48
Q

pH levels

A

Acidic < Neutral (7) < Basic

49
Q

an aqueous solution that resists changes in pH upon the addition of an acid or a base

A

Buffer

50
Q

Buffers constitute

A

a pair of a weak acid and its conjugate base, or a pair of a weak base and its conjugate acid

51
Q

A buffer solution must have

A

a huge concentration of acid to react with any OH- ions that are added to it, and it must contain a similar concentration of base to react with any added H+ ions

52
Q

Buffer (Henderson Hasselbach) Equation

A

pH = pKa + log [A-]/[HA]

or

pH = pKa + log [conjugate base]/[acid]

53
Q

oxidation-reduction (redox) reaction involves the

A

transfer of one or more electrons between reactants

54
Q

Oxidation occurs when

A

an atom loses an electron, resulting to increase in its oxidation state

55
Q

Reduction happens when

A

an atom gains an electron, resulting in the decrease of its oxidation state

56
Q

LEORA

A

Lose Electron(s) - undergoes Oxidation - Reducing Agent

57
Q

GEROA

A

Gain Electron(s) - undergoes Reduction - Oxidizing Agent

58
Q

Electrochemistry

A

the study of the chemical reactions that involve the interconversion between chemical energy and electrical energy

59
Q

An electrochemical cell is a

A

device that can either generate electrical energy from redox reactions or induce redox reactions by using electricity

60
Q

In a galvanic (or voltaic) cell,

A

a spontaneous redox reaction generates the electrical energy

61
Q

Anode and Cathode

A

Oxidation - Anode
Reduction - Cathode

62
Q

Salt-bridge

A

connects two half-cells allows for electrical contact without allowing solutions to mix

63
Q

A negative value of cell potential indicates a reducing environment, while

A

a positive value indicates an oxidizing environment

64
Q

a measure of the tendency of a chemical species to be reduced or to gain electrons

A

Reduction potential

65
Q

the tendency of a chemical species to be oxidized or to give up electrons

A

oxidation potential

66
Q

Cell Potential measured under a standard condition

A

Standard Cell Potential

67
Q

Standard Condition

A
  1. solids and liquids are present in their standard states;
  2. solution concentration is 1M;
  3. temperature is 25° C; and
  4. pressure is atmosphere.
68
Q

The reduction potential measured at standard conditions (the unit is volt, V)

A

Standard reduction potential (E° red)

69
Q

Standard cell potential (E° cell) equation

A

E° cell = E° red(cathode) - E° red(anode)

70
Q

If both the reduction and oxidation potentials of the two half-reactions is considered, then E° cell is

A

E° cell = E° red + E° ox

71
Q

The electrode with the zero potential and from which all other E° red values are based is called the

A

standard hydrogen electrode (SHE)

72
Q

If the calculated cell potential is positive, the reaction is

A

spontaneous

73
Q

If the calculated cell potential is negative, the reaction is

A

non-spontaneous

74
Q

A positive standard cell potential means

A

the cell can generate electricity

75
Q

If the reaction is spontaneous, it is a ________ cell, if it is not, it is considered as an ________ cell

A

galvanic, electrolytic

76
Q

Any battery or cell that we know of are actually ________ cells where the chemical energy from the redox reaction are converted to electrical energy that we can use.

A

galvanic

77
Q

Primary batteries can be used

A

only a certain period of time

78
Q

Secondary batteries can be

A

recharged by applying current and can be used again

79
Q

LeClanche Dry Cell

A

First dry cell. Contains zinc which serves as the anode and a graphite rod at the center which serves as the cathode. In between the electrodes is a paste of zinc chloride (ZnCl2), manganese oxide (Mn02), and ammonium chloride (NH4CI). Cell potential is 1.5V

80
Q

Mercury Button Cell

A

primary cells. They have Zn as an anode and mercury(II) oxide (HgO) as the cathode. Potassium hydroxide (KOH) or sodium hydroxide (NaOH) serves as the electrolyte between the two.
The cell potential is
approximately 1.35V.

81
Q

Fuel Cell

A

Fuel cell is an electrochemical cell that allows the conversion of chemical energy of fuels to electrical energy.
The difference between fuel cells and other form of batteries is that, in fuel cells, the reactants are continuously being supplied in the electrodes and products are continuously removed from the electrolyte compartment.

82
Q

Lead Storage Battery

A

The lead storage battery is one of the most common secondary cell. It is commonly used in automobiles and invertors. It consists of 6 cells that are connected in series and can produce 2V each (12V for the whole Lead
battery).

83
Q

process of degradation of metal due to electrochemical reaction.

A

Corrosion

84
Q

process that can be used to separate a substance into its original components/elements

A

Electrolysis

Gen Chem (4 decks)

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