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Fall 2017 > CHEM 105 Ch. 9-10 > Flashcards

CHEM 105 Ch. 9-10 Flashcards

1
Q

energy

A

anything that has the capacity to do work

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2
Q

work

A

a force acting over a distance (energy = work = force x distance)

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3
Q

heat

A

the flow of energy caused by a difference in temperature

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4
Q

kinetic energy

A

energy of motion or energy that is being transferred

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5
Q

thermal energy

A

energy associated with temperature (a form of kinetic energy)

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6
Q

potential energy

A

energy that is stored in an object or energy associated with the composition and position of the object

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7
Q

energy stored in the structure of a compound is

A

potential energy

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8
Q

chemical energy

A

potential energy due to the structure of the atoms, the attachment between atoms, the atoms’ positions relative to each other in the molecule, or the molecules’ relative positions in the structure

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9
Q

nuclear energy

A

potential energy in the nucleus of atoms

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10
Q

light/radiant energy

A

kinetic energy associated with energy transitions in an atom

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11
Q

heat/thermal energy

A

kinetic energy associated with molecular motion

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12
Q

electrical energy

A

kinetic energy associated with the flow of electrical charge

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13
Q

the amount of kinetic energy an object has is directly proportional to

A

its mass and velocity (KE = 1/2 mv^2)

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14
Q

when the mass is in kg and the velocity is in m/s, the unit for KE is

A 
a joule (J)
1 J = kg*m^2/s^2 = 1 N*m
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15
Q

one joule of energy is the amount of energy needed to move a ? kg mass at a speed of ? m/s

A

1, 1

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16
Q

a calorie (cal) is

A

the amount of energy needed to raise the temperature of 1g water by 1*C

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17
Q

1 kcal = energy needed to

A

raise 1000g water by 1*C

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18
Q

a food Calorie (Cal) is ? calories

A

1000

1 Cal = 1 kcal

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19
Q

1 calorie = ? joules

A

4.184

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20
Q

1 kWh = ? joules

A

3.60 x 10^6

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21
Q

thermodynamics

A

the study of energy that is exchanged between the system and surroundings

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22
Q

the first law of thermodynamics

A

the law of conservation of energy

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23
Q

the law of conservation of energy means that

A

the total amount of energy in the universe is constant; it is conserved (therefore, you can never design a system that will continue to produce energy without some source of energy)

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24
Q

system

A

the part of the universe that is being studied

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25
Q

surroundings

A

everything else in the universe with which the system can exchange energy

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26
Q

when energy flows from the system to the surrounds,

A

the energy of the system decreases, the energy of the surroundings increases; exothermic

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27
Q

when energy flows from the surroundings to the system,

A

the energy of the system increases, the energy of the surroundings decreases; endothermic

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28
Q

conservation of energy means that the amount of energy gained or lost by the system has to be (less than/greater than/equal to) the amount of energy lost or gained by the surroundings

A

equal to

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29
Q

internal energy

A

the sum of the kinetic and potential energy of all the particles that compose the system

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30
Q

the change in the internal energy of a system only depends on

A

the amount of energy in the system at the beginning and end

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31
Q

state function

A

a mathematical function whose result only depends on the initial and final conditions, not on the process used

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32
Q

energy diagram

A

a “graphical” way of showing the direction of energy flow during a process

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33
Q

if the reactants have a lower internal energy than the products, then the change in energy will be

A

positive (endothermic)

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34
Q

if the reactants have a higher internal energy than the products, then the change in energy will be

A

negative (exothermic)

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35
Q

energy is exchanged between the system and surroundings through

A

heat and work

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36
Q

if q (heat) is positive

A

system gains thermal energy

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37
Q

if q (heat) is negative

A

system loses thermal energy

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38
Q

if w (work) is positive

A

work is done on the system

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39
Q

if w (work) is negative

A

work is done by the system

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40
Q

if ΔE (change in internal energy) is positive

A

energy flows into the system

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41
Q

if ΔE (change in internal energy) is negative

A

energy flows out of the system

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42
Q

heat is the exchange of

A

thermal energy between a system and surroundings

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43
Q

heat exchange occurs when

A

system and surroundings have a difference in temperature

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44
Q

temperature

A

the measure of the thermal energy within a sample of matter

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45
Q

heat flows from matter with (low/high) temperature to matter with (low/high) temperature until both objects reach the same temperature (thermal equilibrium)

A

high to low

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46
Q

increase in temperature is directly proportional to ? and the proportionality constant is called the ?

A

the amount of heat absorbed; heat capacity (C)

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47
Q

units for heat capacity (C) are ? and the equation is ?

A

J/*C or J/K

q = cΔT

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48
Q

the larger the heat capacity of the object being studied, the (smaller/larger) the temperature rise will be for a given amount of heat

A

smaller

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49
Q

factors affecting heat capacity

A

amount of matter, type of material

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50
Q

the heat capacity of an object is proportional to

A

its mass and the specific heat of the material

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51
Q

the quantity of heat absorbed by an object can be determined if the following are known with the equation ?

A

mass, specific heat capacity, temperature change

q = m x C x ΔT

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52
Q

specific heat capacity

A

measure of a substance’s intrinsic ability to absorb heat; the amount of heat energy require to raise the temperature of 1g of a substance by 1C; Cs; units J/(gC)

53
Q

the molar heat capacity is

A

the amount of heat required to raise the temperature of one mole of a substance by 1*C

54
Q

? has the highest Cs

A

water (4.18 J/g*C)

55
Q

pressure volume work is caused by

A

a volume change against an external pressure

56
Q

when gases expand, ΔV is (negative/positive), but the system is doing work on the surroundings, so w,gas is (negative/positive)

A

positive, negative

57
Q

as long as the external pressure is kept constance, w =

A

-PΔV

58
Q

1 atm * L = ? J

A

101.3 J

59
Q

exchange of heat energy equation, exchange of work equation

A 
q = mCΔT
w = -PΔV
60
Q

at constant volume, ΔEsystem =

A

q,system

61
Q

in practice, temperature changes of individual chemicals involved in the reaction cannot be observed directly, so instead the ? in surroundings is measured using ?, so ?

A

ΔT, an insulated container, q,system = -q,surroundings

62
Q

bomb calorimeter

A

used to measure ΔE because it is a constant volume system; the heat capacity of the calorimeter is the amount of heat absorbed by the calorimeter for each degree rise in temp. and is called the calorimeter constant

63
Q

enthalpy, H, of a system

A

the sum of the internal energy of the system and the prouct of pressure and volume; a state function; H = E + PV

64
Q

the enthalpy change, ΔH, of a reaction

A

the heat evolved in a reaction at constant pressure; ΔH,reaction = q,reaction at constant pressure

65
Q

when ΔH is negative,

A

heat is being released by the system into the surroundings; exothermic

66
Q

when ΔH is positive,

A

heat is being absorbed by the system from the surroundings; endothermic

67
Q

the enthalpy of change in a chemical reaction is an ? property, meaning

A

extensive; dependent on the amount (i.e., more reactions => larger enthalpy change)

68
Q

by convention, we calculate the enthalpy change for the number of moles of reactants in the reactions…

A

as written

69
Q

ΔHreaction =

A

q,constant pressure = q,reaction

70
Q

to get ΔHreaction per mole of a particular reactant,

A

divide by the number of moles that reacted then multiply by the coefficient in the equation

71
Q

Hess’s Law

A

the change in enthalpy for a step-wise process is the sum of the enthalpy changes of the steps

72
Q

ΔHreaction can be estimated by comparing the cost of

A

breaking old bonds to the income from making new bonds

73
Q

bond energy

A

the amount of energy it takes to break one mole of a bond in a compound

74
Q

ΔHreaction = (in terms of bond energies)

A

Σ(ΔH(bonds broken)) + Σ(ΔH(bonds formed))

75
Q

the more e-s two atoms share, the ? the covalent bond (must be comparing bonds b/w like atoms)

A

stronger

76
Q

the shorter the covalent bond, the ? the covalent bond (must be comparing similar types of bonds) because…

A

stronger; bonds get weaker down the column and stronger across the period (atomic radii decrease across the period and increase down the column)

77
Q

standard state

A

state of a material at a defined set of conditions

78
Q

the standard enthalpy change, ΔH*, is the enthalpy change when

A

all reactants and products are in their standard states

79
Q

standard state for gas

A

1 atm pressure

80
Q

standard state for solid or liquid

A

1 atm pressure, usually 25*C temperature

81
Q

standard state for substance in solution

A

concentration 1 M

82
Q

the ΔH*,f for a pure element in its standard state

A

0 kJ/mol

83
Q

ΔH*,rxn = (in terms of standard enthalpy)

A

Σ(nΔH,f(products)) - Σ(nΔH,f(reactants))

where n is the coefficient for each product or reactant

84
Q

crystal lattice

A

structure formed by an ionic solid in which every cation is surrounded by anions and vice versa; maximized the attractions b/w cations and anions, leading to the most stable arrangement; held together by the electrostatic attraction of the cations for all the surrounding anions

85
Q

lattice energy

A

the extra stability that accompanies the formation of the crystal lattice; the energy released when the solid crystal forms from separate ions in the gas state (always exothermic); depends directly on the size of charges and inversely on distance b/w ions

86
Q

Born-Haber cycle

A

a hypothetical series of reactions that represents the formation of an ionic compound from its constituent elements

87
Q

the reactions in the Born-Haber cycle are chosen so that

A

the change in enthalpy of each reaction is known except for the last one, which is the lattice energy

88
Q

how to use the Born-Haber cycle and Hess’s law to calculate lattice energy

A

use Hess’s law to add up enthalpy changes of other reactions to determine lattice energy

89
Q

ΔH*(crystal lattice) =

A

lattice energy

90
Q

ΔH*(metal atom (g)) =

A

first ionization energy

91
Q

ΔH*(nonmetal atom (g)) =

A

electron affinity

92
Q

trends in lattice energy

A

ion size and ion charge (more important)

93
Q

the force of attraction between charged particles is (directly/inversely) proportional to the distance between them

A

directly (this is Coulomb’s Law: q1q2/r)

94
Q

a gaseous atom or molecule exerts a force when it collides with

A

a surface or other gaseous particles (molecular collisions are pressure)

95
Q

gas pressure

A

the force exerted per unit area by gas molecules as they strike surfaces around them (P = F/A); a result of the constant movement of the gas molecules and their collisions with the surfaces around them

96
Q

the pressure of a gas depends on

A

the number of gas particles in a given volume, the volume of the container, and the average speed of the gas particles

97
Q

according to the Kinetic Theory of Gases, collisions of gas particles with each other and/or surfaces are said to be ?, meaning ?

A

elastic, meaning no exchange of energy occurs

98
Q

pressure (decreases/increases) with a higher concentration of gas molecules

A

increases

99
Q

pressure is (low/high) with a low number of gas particles in a given volume

A

low

100
Q

as volume increases, the concentration of gas molecules (decreases/increases)

A

decreases

101
Q

1 mmHg = ? torr

A

1 torr

102
Q

1 atm = ? mmHg = ? torr

A

760

103
Q

1 atm = ? bar

A

1.013

104
Q

1 atm = ? Pa

A

101325

105
Q

1 atm = ? Psi

A

14.7

106
Q

1 atm = ? in Hg

A

29.92

107
Q

how manometers work

A

the difference in liquid levels is a measure of the difference in pressure between gas and atmosphere (if atmosphere side higher, gas has higher pressure b/c pushing liquid that way)

108
Q

4 basic properties of gases and their units

A
  1. pressure (atm)
  2. volume (L)
  3. temperature (K)
  4. amount in moles (n)
109
Q

Boyle’s Law

A

pressure and volume are inversely related (P1V1 = P2V2)

110
Q

Charles’s Law

A

volume and temperature are directly related (V1/T1 = V2/T2)

111
Q

Avogadro’s Law

A

volume is directly proportional to the number of gas molecules (V1/n1 = V2/n2)

112
Q

Ideal Gas Law

A 
PV = nRT, where
P = pressure in atm
V = volume in L
n = # moles
R = constant (0.0821 L*atm/mol*K)
T = temperature in K
113
Q

standard conditions

A 
P = 1 atm
T = 273K = 0*C
n = 1 mol
V = 22.4 L
114
Q

density of a gas

A

molar mass of gas (g/mol) / molar volume (L/mol)

molar volume = 22.4 L

115
Q

molar mass of a gas

A

mass (g) / mole (n)

116
Q

gas density from PV=nRT

A 
d = PM / RT
(M = molar mass; can use n = mass (g) / M)
117
Q

dry air is composed of

A

nitrogen, oxygen, argon, carbon dioxide, and a few other gases

118
Q

Dalton’s Law

A

total pressure of a gas mixture = sum of partial pressures

119
Q

particles with different masses have (the same/different) kinetic energies at a given temperature

A

the same

120
Q

partial pressure of a gas

A

the pressure of a single gas in a mixture of gases

121
Q

partial pressure can be calculated if

A

1) a fraction of the mixture it composes and the total pressure are known
2) the number of moles of the gas in a container of a given volume and temperature is known

122
Q

partial pressure equation

A

Pn = n,n * (R*T / V) or X,a * P,total

123
Q

total pressure from partial pressures equation

A

P,total = n,total * (R*T / V)

124
Q

mole fraction, X,a

A

the ratio of the partial pressure a single gas contributes to the total pressure; X,a = P,a / P,total = n,a / n,total

125
Q

deep sea diving and oxygen levels

A

abnormally high partial pressure of O2 => elevated concentration of oxygen in body tissues; safe range is between 0.21 and 1.4

126
Q

collecting gases by displacing water from a container

A

get the gas + water vapor (the partial pressure of the water vapor depends on temperature only)

127
Q

Kinetic Molecular Theory

A

the simplest model for the behavior of gases; a gas is modeled as a collection of particles in constant motion; the average KE of the gas particles is directly proportional to the Kelvin temperature; collisions completely elastic

128
Q

postulates of the KMT

A

the particles of the gas are constantly moving, the attraction b/w particles is negligible, collisions => bounce off & keep moving, lots of empty space b/w gas particles compared to size of particles

129
Q

chapter ten

A

continued

Fall 2017 (24 decks)

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