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Chemistry > Chapter 7- Energy, Rate & Equilibrium > Flashcards

Chapter 7- Energy, Rate & Equilibrium Flashcards

(91 cards)

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0
Q

Can be applied to the study of chemical or physical changes

A

Thermodynamics

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1
Q

The study of energy, work, and heat

A

Thermodynamics

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2
Q

Adding energy (in the form of heat or work) __ __

A

Breaks bonds

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3
Q

New bonds may form resulting in new products, __ energy

A

Releasing

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4
Q

It is difficult to measure an absolute value for energy stores in a ___ system

A

Chemical

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5
Q

It is much simpler to measure a change in energy __( )__ as a chemical reaction occurs

A

(Delta E)

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6
Q

Contains the process under study

A

System

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7
Q

Encompasses the rest of the universe

A

Surroundings

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8
Q

Energy can be ___ by the system from the surroundings or lost from the system to the ___

A

Gained

Surroundings

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9
Q

Energy cannot be created or destroyed, only converted from one form to another

A

Law of thermodynamics

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10
Q

The universe spontaneously tends toward increasing entropy

A

Law of thermodynamics

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11
Q

The entropy is a pure perfect crystal at absolute zero is zero

A

Law of thermodynamics

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12
Q

Releases energy to the surroundings

A

Exothermic reaction

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13
Q

In an exit hermit reaction the energy required to break the bonds is ___ than the energy given off when the bonds form

A

Less

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14
Q

Absorbs energy from the surroundings

A

Endothermic reaction

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15
Q

In an endothermic reaction the energy required to break the bonds is ___ than the energy released when the bonds form

A

Greater

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16
Q

Fuel oil is burned in a furnace

A

Exothermic

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17
Q

When solid NaOH is dissolved in water, the solution temperature increases

A

Exothermic

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18
Q

Liquid water vaporizes into gaseous water

A

Endothermic

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19
Q

A function representing heat under conditions of constant pressure (containers open to the atmosphere)

A

Enthalpy

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20
Q

Change in enthalpy -(__)- the energy __ between the products and reactants of a chemical reaction

A

(Delta H)

Difference

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21
Q

Energy released

A

Exothermic reaction

(Delta H) is negative

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22
Q

Energy absorbed

A 
Endothermic reaction 
(Delta H) is positive
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23
Q

Many Exothermic reactions are

A

Spontaneous

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24
Most endothermic reactions are
Nonspontaneous
25
The measure of the statistical distribution of energy in a system
Entropy
26
Energy very well distributed
High entropy
27
Energy not very well spread out
Low entropy
28
The difference of entropies a of states
Gases>liquids>solids
29
A function that considers both the enthalpy and entropy of a system
Gibbs free energy (G)
30
Delta H- T•Delta S
Equation for Gibbs free energy
31
If delta G<0 then the process releases free energy to the surroundings and the process is
Spontaneous
32
If Delta G> 0 then the process consumes free energy and will __ occur spontaneously
Not
33
The measurement of heat energy changes in a chemical reaction
Calorimetry
34
The amount of heat (calories or Joules) needed to raise the temperature of 1 gram of the substance 1 degree Celsius
Specific Heat (Cs)
35
Q= ms* delta Ts * Cs
Equation for calorimetry
36
The amount of energy per gram of food
Fuel value
37
Fuel value or reported in units of nutritional
Calories
38
1 Cal=
1000 cal
39
The study of the rate (or speed) of chemical reactions
Chemical kinetics
40
Gives an indication of the mechanism of a reaction
Chemical kinetics
41
A step by step description of how reactants become products
Mechanism
42
Expressed as the disappearance of reactants or appearance of product over time
Chemical kinetics
43
The min amount of energy requires to initiate a chemic reaction
Activation energy
44
Reaction proceeds from reactants to products through a high stat called the __ __ or transition state
Activated complex
45
Difference between the energy of the reactants and the activated complex is the
Activation energy
46
A higher activation energy leads to a slower
Reaction rate
47
Factors influencing reaction rate
``` Structure of reacting species Molecular shape and orientation Concentration of reactants Temperature of reactants Physical state of reactants Presence of a catalyst ```
48
__ charged species react more rapidly
Oppositely
49
Ions with the same charge __
Repel
50
For covalent molecules , some bonds must be broken ( ) before new bonds can be formed
Activation energy
51
Magnitude of the activation energy is related to the ___ of the bonds that must be broken
Strength
52
Large molecules may ___ the reactive part of the molecule
Obstruct
53
Only molecular collisions with correct ___ lead to product formation
Orientation
54
Rate is related to the concentration of one or more of the
Reacting substances
55
Rate will generally ___ as concentration increases
Increase
56
Higher concentration means __ reactant molecules per unit volume
More
57
More reactant molecules means more ___ per unit time
Collisions
58
Rate ___ as temp increases
Increases
59
Faster particles increases likelihood of
Collision
60
Higher kinetic energy means a higher percentage of these collisions will result in product
Formation
61
Reactions occur when reactants can collide frequently with sufficient ___ to react
Energy
62
Rate of states
Liquid >gas> solid
63
A catalyst is ___ ___ during a reaction
Not changed
64
A catalyst does not alter the final ___ of the reaction
Product
65
A catalyst interacts with the reactants to create an ___ ___ for product production
Alternative mechanism
66
We use catalyst to __ up a reaction
Speed
67
A catalyst ___ the activation energy you need so the reaction happens faster
Lowers
68
A chemical reaction that does not go to completion
Equilibrium reaction
69
A process that can occur in both directions; indicated by a double arrow symbol
Reversible reaction
70
A situation in which the rate of the forward process in a reversible reaction is exactly balanced by the rate of the reverse process
Dynamic equilibrium
71
Sugar (s) --> sugar (aq)
Reaction goes to completion
72
Sugar (s) --> <-- sugar (aq)
Rates are equal, not percentages
73
Rates of the forward and reverse reactions are equal
Chemical equilibrium
74
Products are being consumed and formed at the same rate
Chemical equilibrium
75
Equilibrium constant expression can be written to summarize the relationship between the concentration of reactants and products
Chemical equilibrium
76
Equilibrium constant expression
Keq= [C]^c[D]^d/[A]^a[B]^b
77
The numerical value of the equilibrium constant tells the extent to which reactants have been converted to
Products
78
Keq greater than 100 at equilibrium
Mostly product is present
79
Keq less than 0.01 at equilibrium
Mostly reactant is present
80
Keq between 0.01-100 at equilibrium
The mixture contains significant concentrations of both reactants and products
81
States that if a stress is placed on a system at equilibrium, the system will respond by altering the equilibrium composition in such a way as to minimize that stress
LeChatelier's principle
82
Product introduced
Equilibrium shifts to the left
83
Reactant introduced
Equilibrium shifts the the right
84
Product taken out
Equilibrium shifts right
85
Reactant taken out
Equilibrium shifts left
86
If its an Exothermic reaction and temperature is increased
Equilibrium shifts left
87
If endothermic reaction and temp is increased
Equilibrium shifts right
88
If gas is reactant and pressure is increased
Equilibrium shifts left
89
If gas is product and pressure is increased
Equilibrium shifts left
90
Catalysts do __ affect the position of equilibrium
Not

Chemistry (3 decks)

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