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

Chapter 7- Energy, Rate & Equilibrium Flashcards

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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
Q

Most endothermic reactions are

A

Nonspontaneous

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25
Q

The measure of the statistical distribution of energy in a system

A

Entropy

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26
Q

Energy very well distributed

A

High entropy

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27
Q

Energy not very well spread out

A

Low entropy

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28
Q

The difference of entropies a of states

A

Gases>liquids>solids

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29
Q

A function that considers both the enthalpy and entropy of a system

A

Gibbs free energy (G)

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30
Q

Delta H- T•Delta S

A

Equation for Gibbs free energy

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31
Q

If delta G<0 then the process releases free energy to the surroundings and the process is

A

Spontaneous

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32
Q

If Delta G> 0 then the process consumes free energy and will __ occur spontaneously

A

Not

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33
Q

The measurement of heat energy changes in a chemical reaction

A

Calorimetry

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34
Q

The amount of heat (calories or Joules) needed to raise the temperature of 1 gram of the substance 1 degree Celsius

A

Specific Heat (Cs)

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35
Q

Q= ms* delta Ts * Cs

A

Equation for calorimetry

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36
Q

The amount of energy per gram of food

A

Fuel value

37
Q

Fuel value or reported in units of nutritional

A

Calories

38
Q

1 Cal=

A

1000 cal

39
Q

The study of the rate (or speed) of chemical reactions

A

Chemical kinetics

40
Q

Gives an indication of the mechanism of a reaction

A

Chemical kinetics

41
Q

A step by step description of how reactants become products

A

Mechanism

42
Q

Expressed as the disappearance of reactants or appearance of product over time

A

Chemical kinetics

43
Q

The min amount of energy requires to initiate a chemic reaction

A

Activation energy

44
Q

Reaction proceeds from reactants to products through a high stat called the __ __ or transition state

A

Activated complex

45
Q

Difference between the energy of the reactants and the activated complex is the

A

Activation energy

46
Q

A higher activation energy leads to a slower

A

Reaction rate

47
Q

Factors influencing reaction rate

A 
Structure of reacting species 
Molecular shape and orientation 
Concentration of reactants 
Temperature of reactants
Physical state of reactants 
Presence of a catalyst
48
Q

__ charged species react more rapidly

A

Oppositely

49
Q

Ions with the same charge __

A

Repel

50
Q

For covalent molecules , some bonds must be broken ( ) before new bonds can be formed

A

Activation energy

51
Q

Magnitude of the activation energy is related to the ___ of the bonds that must be broken

A

Strength

52
Q

Large molecules may ___ the reactive part of the molecule

A

Obstruct

53
Q

Only molecular collisions with correct ___ lead to product formation

A

Orientation

54
Q

Rate is related to the concentration of one or more of the

A

Reacting substances

55
Q

Rate will generally ___ as concentration increases

A

Increase

56
Q

Higher concentration means __ reactant molecules per unit volume

A

More

57
Q

More reactant molecules means more ___ per unit time

A

Collisions

58
Q

Rate ___ as temp increases

A

Increases

59
Q

Faster particles increases likelihood of

A

Collision

60
Q

Higher kinetic energy means a higher percentage of these collisions will result in product

A

Formation

61
Q

Reactions occur when reactants can collide frequently with sufficient ___ to react

A

Energy

62
Q

Rate of states

A

Liquid >gas> solid

63
Q

A catalyst is ___ ___ during a reaction

A

Not changed

64
Q

A catalyst does not alter the final ___ of the reaction

A

Product

65
Q

A catalyst interacts with the reactants to create an ___ ___ for product production

A

Alternative mechanism

66
Q

We use catalyst to __ up a reaction

A

Speed

67
Q

A catalyst ___ the activation energy you need so the reaction happens faster

A

Lowers

68
Q

A chemical reaction that does not go to completion

A

Equilibrium reaction

69
Q

A process that can occur in both directions; indicated by a double arrow symbol

A

Reversible reaction

70
Q

A situation in which the rate of the forward process in a reversible reaction is exactly balanced by the rate of the reverse process

A

Dynamic equilibrium

71
Q

Sugar (s) –> sugar (aq)

A

Reaction goes to completion

72
Q

Sugar (s) –> <– sugar (aq)

A

Rates are equal, not percentages

73
Q

Rates of the forward and reverse reactions are equal

A

Chemical equilibrium

74
Q

Products are being consumed and formed at the same rate

A

Chemical equilibrium

75
Q

Equilibrium constant expression can be written to summarize the relationship between the concentration of reactants and products

A

Chemical equilibrium

76
Q

Equilibrium constant expression

A

Keq= [C]^c[D]^d/[A]^a[B]^b

77
Q

The numerical value of the equilibrium constant tells the extent to which reactants have been converted to

A

Products

78
Q

Keq greater than 100 at equilibrium

A

Mostly product is present

79
Q

Keq less than 0.01 at equilibrium

A

Mostly reactant is present

80
Q

Keq between 0.01-100 at equilibrium

A

The mixture contains significant concentrations of both reactants and products

81
Q

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

A

LeChatelier’s principle

82
Q

Product introduced

A

Equilibrium shifts to the left

83
Q

Reactant introduced

A

Equilibrium shifts the the right

84
Q

Product taken out

A

Equilibrium shifts right

85
Q

Reactant taken out

A

Equilibrium shifts left

86
Q

If its an Exothermic reaction and temperature is increased

A

Equilibrium shifts left

87
Q

If endothermic reaction and temp is increased

A

Equilibrium shifts right

88
Q

If gas is reactant and pressure is increased

A

Equilibrium shifts left

89
Q

If gas is product and pressure is increased

A

Equilibrium shifts left

90
Q

Catalysts do __ affect the position of equilibrium

A

Not

Chemistry (3 decks)

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