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Gen Chem > Lesson 6-10 > Flashcards

Lesson 6-10 Flashcards

(84 cards)

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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
The DEGREE OF DISORDERLINESS (ENTROPY) of a simple substance can generally be determined by
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.
26
Factors that combine to predict spontaneity
Energy Change, Temperature, Entropy Change
27
A reaction will ________ spontaneously move away from equilibrium and will always move spontaneously ________ equilibrium.
Never, Towards
28
A reaction that does occur under a given set of conditions is called
spontaneous reaction
29
If G is positive, then
the reaction is nonspontaneous
30
A reaction is at ________ state if the rate of the forward reaction equals the rate of the backward reaction.
equilibrium
31
mA + nB -> xC + yD
Qc = [(C^x) * (D^y)] / [(A^m) * (B^n)]
32
If Qc < Kc, then
The reaction proceeds on a forward direction
33
If Qc > Kc
Reaction proceeds on a reverse direction
34
If Qc = Kc
Reaction is at equilibrium
35
reactions in which all reacting species are in the same phase.
homogeneous equilibrium
36
aA + bB ⇌ cC + dD
Kc = [(C^c) * (D^d)] / [(A^a) * (B^b)]
37
Le Chatelier's Principle, states that
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
adding additional reactant to a system will shift the equilibrium to the
right, towards the side of the products
39
Catalysts has ____________ on the equilibrium system
no effect
40
Brensted-Lowry theory describes
acid-base interactions in terms of proton transfer between chemical species
41
Bronsted acid is a
substance capable of donating a proton (H+ ions)
42
Bronsted base is a
substance capable of accepting a proton (H+ ions)
43
conjugate acid-base pair which can be defined as
an acid and its conjugate base or a base and its conjugate acid
44
product formed when acid loses H+
Conjugate base
45
product formed when base gains H+
Conjugate acid
46
pH formula
pH = -log[H+]
47
pH meaning
Power of Hydrogen, negative logarithm of the hydrogen ion concentration
48
pH levels
Acidic < Neutral (7) < Basic
49
an aqueous solution that resists changes in pH upon the addition of an acid or a base
Buffer
50
Buffers constitute
a pair of a weak acid and its conjugate base, or a pair of a weak base and its conjugate acid
51
A buffer solution must have
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
Buffer (Henderson Hasselbach) Equation
pH = pKa + log [A-]/[HA] or pH = pKa + log [conjugate base]/[acid]
53
oxidation-reduction (redox) reaction involves the
transfer of one or more electrons between reactants
54
Oxidation occurs when
an atom loses an electron, resulting to increase in its oxidation state
55
Reduction happens when
an atom gains an electron, resulting in the decrease of its oxidation state
56
LEORA
Lose Electron(s) - undergoes Oxidation - Reducing Agent
57
GEROA
Gain Electron(s) - undergoes Reduction - Oxidizing Agent
58
Electrochemistry
the study of the chemical reactions that involve the interconversion between chemical energy and electrical energy
59
An electrochemical cell is a
device that can either generate electrical energy from redox reactions or induce redox reactions by using electricity
60
In a galvanic (or voltaic) cell,
a spontaneous redox reaction generates the electrical energy
61
Anode and Cathode
Oxidation - Anode Reduction - Cathode
62
Salt-bridge
connects two half-cells allows for electrical contact without allowing solutions to mix
63
A negative value of cell potential indicates a reducing environment, while
a positive value indicates an oxidizing environment
64
a measure of the tendency of a chemical species to be reduced or to gain electrons
Reduction potential
65
the tendency of a chemical species to be oxidized or to give up electrons
oxidation potential
66
Cell Potential measured under a standard condition
Standard Cell Potential
67
Standard Condition
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
The reduction potential measured at standard conditions (the unit is volt, V)
Standard reduction potential (E° red)
69
Standard cell potential (E° cell) equation
E° cell = E° red(cathode) - E° red(anode)
70
If both the reduction and oxidation potentials of the two half-reactions is considered, then E° cell is
E° cell = E° red + E° ox
71
The electrode with the zero potential and from which all other E° red values are based is called the
standard hydrogen electrode (SHE)
72
If the calculated cell potential is positive, the reaction is
spontaneous
73
If the calculated cell potential is negative, the reaction is
non-spontaneous
74
A positive standard cell potential means
the cell can generate electricity
75
If the reaction is spontaneous, it is a ________ cell, if it is not, it is considered as an ________ cell
galvanic, electrolytic
76
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.
galvanic
77
Primary batteries can be used
only a certain period of time
78
Secondary batteries can be
recharged by applying current and can be used again
79
LeClanche Dry Cell
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
Mercury Button Cell
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
Fuel Cell
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
Lead Storage Battery
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
process of degradation of metal due to electrochemical reaction.
Corrosion
84
process that can be used to separate a substance into its original components/elements
Electrolysis

Gen Chem (4 decks)

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