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Chemistry for Engineers > FINALS > Flashcards

FINALS Flashcards

1
Q

the ability to do work or transfer heat

A

energy

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2
Q

the study of energy and its transformation

A

thermodynamics

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3
Q

the study of chemical reactions and the energy changes that involve heat

A

thermochemistry

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4
Q

seen between oppositely charged ions

A

electrostatic attraction

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5
Q

chemical bonds are formed

A

energy is released

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6
Q

when chemical bonds are broken

A

energy is consumed

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7
Q

can be converted from one form to another, but it is neither created nor destroyed

A

energy

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8
Q

portion of the universe that we single out study

A

system

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9
Q

are everything else

A

surroundings

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10
Q

TYPES OF SYSTEM

A

Open, Closed, Isolated

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11
Q

can exchange heat and mass with its surroundings

A

open system

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12
Q

can only exchange heat with its surroundings

A

closed system

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13
Q

can not exchange heat or mass with its surroundings

A

isolated system

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14
Q

system is the sum of all kinetic and potential energies of all components

A

internal energy

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15
Q

system absorbed energy from the surroundings.

A

ΔE > 0, Efinal > Einitial

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16
Q

the system released energy to the surroundings.

A

ΔE < 0, Efinal < Einitial

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17
Q

What is the value of ΔE if Efinal equals Einitial?

A

zero

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18
Q

three parts of thermodynamic quantities

A

number, unit, sign

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19
Q

the system gains energy from the surroundings.

A

A positive ΔE

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20
Q

the system loses energy to the surroundings.

A

negative ΔE

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21
Q

change of internal energy is:

A

ΔE = q + w

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22
Q

heat is absorbed by the system from the surroundings

A

endothermic

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23
Q

heat is released by the system into the surroundings

A

exothermic

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24
Q

internal energy is a

A

state function

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25
Q

change of internal energy depends on the

A

initial and final internal energy

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26
Q

the only work done by chemical or physical change is

A

mechanical work

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27
Q

what is the formula of work

A

w = -PΔV

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28
Q

work done by the system

A

work is negative

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29
Q

the internal energy plus the product of pressure and volume

A

enthalphy

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30
Q

formula of enthalphy is

A

H = E+PV

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31
Q

the change in enthalphy is the heat gained or lost

A

at constant pressure

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32
Q

a process is ____ when change of enthalphy is positive

A

endothermic

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33
Q

A process is_____when ΔH is negative.

A

exothermic

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34
Q

the formula of change in enthalphy

A

ΔHrxn = Hproducts − Hreactants

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35
Q

ΔHrxn

A

enthalpy of reaction, or the heat of reaction.

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36
Q

an extensive property

A

enthalphy

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37
Q

the enthalphy change for a reaction is equal in __ but opposite in sign

A

magnitude

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38
Q

the enthalpy change for the reaction in which a compound is made from its constituent elements in their elemental forms.

A

enthalphy of formation

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39
Q

The enthalpy associated with breaking one mole of a particular bond in a gaseous substance.

A

bond enthalphy

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39
Q

the bond enthalphy is always ___ because energy is required to break chemical bonds

A

positive

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39
Q

always released when a bond forms

A

energy

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40
Q

the greater the bond enthalphy

A

the stronger the bond

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41
Q

the measurement of heat flow

A

calorimetry

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42
Q

instrument used to measure heat flow

A

calorimeter

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43
Q

amount of energy required to raise the temperature of a substance

A

heat capacity

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44
Q

energy released when one gram of food is combusted

A

fuel value

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45
Q

composed of the two nucleons, protons and neutrons

A

nucleus

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46
Q

is the atomic number

A

number of protons

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47
Q

the number of protons and neutrons together

A

mass number

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48
Q

not all atoms of the same element have the same mass due to different numbers of neutrons in those atoms

A

isotopes

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49
Q

Some nuclei change spontaneously, emitting radiation. They are said to be

A

radioactive

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49
Q

three naturally occuring isotopes of uranium

A

Uranium 234, 235, 238

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50
Q

We use nuclear equations to show

A

how these nuclear reactions occur.

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51
Q

atoms and charges need to balance

A

In chemical equations

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52
Q

the loss of a γ-ray, which is high-energy radiation

A

gamma emission

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52
Q

atomic number and mass number need to balance

A

In nuclear equations

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53
Q

Types of Radioactive Decay

A

Alpha decay
Beta decay
Gamma emission
Positron emission
Electron capture

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54
Q

the loss of an α-particle (He-4 nucleus, two protons and two neutrons):

A

Alpha decay

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54
Q

the loss of a β-particle (a high-speed electron emitted by the nucleus

A

Beta Decay

55
Q

a particle that has the same mass as, but an opposite charge to, that of an electron:

A

positron emission

56
Q

some nuclei decay by emitting a

A

positron

57
Q

An electron from the surrounding electron cloud is absorbed into the nucleus during

A

Electron Capture

58
Q

What change in the mass number of a nucleus occurs when the nucleus emits an alpha particle?

A

-4

59
Q

Which type of radioactive decay converts a neutron into a proton?

A

Beta Decay

60
Q

is the time required for half of a radionuclide sample to decay.

A

half-life

61
Q

are radioisotopes used to study a chemical reaction.

A

radiotracers

62
Q

react chemically exactly the same as nonradioactive nuclei of the same element.

A

radionuclides

63
Q

A compound labeled with a positron emitter is injected into a patient.

A

Positron emission tomography

64
Q

is used to study the brain, as seen in the figure to the right.

A

labeled glucose

65
Q

einstein’s famous equation is

A

E = mc^2

66
Q

is associated with making and breaking chemical bonds.

A

chemical energy

67
Q

is due to changes in the nucleus of atoms changing them into different atoms

A

nuclear energy

68
Q

released in the transmutation strike other nuclei, causing their decay and the production of more neutrons

A

neutrons

69
Q

The minimum mass that must be present for a chain reaction to be sustained

A

critical mass

70
Q

If more than critical mass is present, an explosion will occur

A

supercritical mass

71
Q

When small atoms are combined, much energy is released. This occurs on the Sun. The reactions are often called

A

thermonuclear reactions

72
Q

is more harmful to living systems than nonionizing radiation

A

ionizing radiation

73
Q

the study of the relationships between electricity and chemical reactions.

A

electrochemistry

74
Q

To keep track of what loses electrons and what gains them

A

oxidation numbers

75
Q

If the oxidation number increases for an element, that element is

A

iodized

76
Q

If the oxidation number decreases for an element, that element is

A

reduced

77
Q

A species is ____ when it loses electrons

A

oxidized

78
Q

A species is____ when it gains electrons.

A

reduced

79
Q

In spontaneous redox reactions, ____ are transferred and ______ is released.

A

electrons, energy

80
Q

energy can do work if the electrons flow through an external device.

A

voltaic cell

81
Q

The oxidation occurs at the

A

anode.

82
Q

The reduction occurs at the

A

cathode

83
Q

In the cell, _____ leave the anode and flow through the wire to the ______

A

electrons, cathode

83
Q

As the electrons reach the cathode, ______ in solution are attracted to the now _____ cathode.

A

cations, negative

83
Q

electromotive force is also called

A

cell potential

83
Q

are formed in the anode compartment.

A

cation

84
Q

The potential difference between the anode and cathode in a cell

A

electromotive force (emf)

84
Q

the greater the tendency for reduction under standard conditions.

A

The more positive the value of E°red

84
Q

electromotive force is measured in ?

A

volts (V)

85
Q

have the most positive reduction potentials

A

the strongest oxidizers

86
Q

have the most negative reduction potentials

A

the strongest reducers

87
Q

Notice that the Nernst equation implies that a cell could be created that has the same substance at both electrodes,

A

concentration cell

88
Q

cannot be recharged when “dead”—the reaction is complete

A

primary cells

88
Q

the measure of spontaneity, positive emf corresponds to negative ΔG.

A

Gibbs free energy

88
Q

a portable, self-contained electrochemical power source that consists of one or more voltaic cells

A

batteries

88
Q

can be recharged

A

secondary cells

89
Q

reactants and products are solids

A

Lead- acid battery

90
Q

most common primary battery

A

alkaline battery

91
Q

kinds of batteries that are lightweight and rechargeable

A

Ni-Cd and Ni-metal hybride batteries

92
Q

Cd is considered as ?

A

toxic and heavy

93
Q

rechargeable, light; produce more voltage than Ni-based batteries.

A

Lithium- ion batteries

94
Q

The direct conversion of chemical to electrical energy is expected to be more efficient and is the basis for

A

fuel cells

94
Q

When a fuel is ____, the energy created can be converted to electrical energy.

A

burned

95
Q

fuel batteries are not batteries

A

true

96
Q

corrosion is

A

oxidation

97
Q

common name of corrosion is

A

rusting

97
Q

occurs because zinc is more easily oxidized

A

Cathodic protection

97
Q

is attached to the pipe. The anode is oxidized before the pipe.

A

Sacrificial Anode

97
Q

Nonspontaneous reactions can occur in electrochemistry IF _____ electricity is used to drive the reaction.

A

outside

97
Q

Use of electrical energy to create chemical reactions is

A

electrolysis

97
Q

the least weighty part of the environment, but it is complex and has a disproportionately large influence on our planet.

A

atmosphere

97
Q

total mass of the atmosphere is estimated to be around

A

5.15 x 10^18 kg

98
Q

arose from the out-gassing of Earth when it was simply a molten mass

A

nitrogen

98
Q

is not the direct source of this element in living beings

A

Gaseous N2

98
Q

nitrogen must be in the form of a usable nitrogen compound, such as

A

ammonia, ammonium or nitrate ions

99
Q

who are the two geman chemists who devised a way to transform nitrogen in the air into fertilizer?

A

Fritz Haber and Carl Bosch

100
Q

The nitrogen cycle involves nitrogen fixation by soil bacteria or, in aquatic environments, by

A

cyanobacteria

101
Q

ions produced are converted to nitrate ions, the main form of nitrogen absorbed by plants

A

NH4+

101
Q

is the second most abundant species present in the atmosphere.

A

O2

102
Q

is by-product of plant photosynthesis

A

oxygen

102
Q

first began producing oxygen as long ago as 3.5 billion years.

A

Blue-green algae, or cyanobacteria

103
Q

Nitrogen is returned to the atmosphere by ____ which convert nitrate ions to n2

A

denitrifying bacteria

104
Q

a microbial process by which reduced nitrogen compounds (primarily ammonia) are sequentially oxidized to nitrite and nitrate.

A

Nitrification

104
Q

a chemicalprocess that intends to “lock” tissue, cells, and subcellular components as close as possible to its original status

A

Fixation

105
Q

acts as a shield from the UV- rays in stratosphere

A

Ozone (O3)

105
Q

it is also a pollutant in troposphere

A

Ozone (O3)

105
Q

The leakage of chlorofluorocarbons CFCs in refrigerators and other domestic appliance causes the depletion of ozone layer.

A

ozone hole

106
Q

the two molecule are

A

CFC-114 (C2Cl2F4) and CFC-12 (CCl2F2)

106
Q

CFC 114

A

Dichlorotetrafluoroethane

106
Q

CFC-12 (CCl2F2)

A

Dichlorodifluoromethane

106
Q

has the ability to form stable compounds consisting of long chains and rings of atoms.

A

carbon

107
Q

the basis of the structures for many compounds that comprise the living cell.

A

carbon

108
Q

The food we eat—carbohydrates, oils, proteins, and fiber—is made up of compounds of

A

carbon

108
Q

name given to the trapping of energy in the Earth’s atmosphere by a process very similar to that occurring in glass-enclosed greenhouses in which plants are grown

A

greenhouse effect

109
Q

The greenhouse effect is caused by certain gases in the troposphere called

A

greenhouse gases

110
Q

These gases are small molecules whose bonds vibrate with frequencies in the infrared region of the electromagnetic spectrum (resonance phenomena).

A

greenhouse gases

111
Q

primary greenhouses gases are:

A

Water vapor H2O
Carbon dioxide CO2
Nitrous oxide N2O

112
Q

the main greenhouse gas and accounts for most of the observed effect.

A

water vapor

112
Q

a comprehensive air quality management policy and program which aims to achieve and maintain healthy air for all Filipinos.

A

Republic Act No. 8749 or Philippine Clean Air Act

112
Q

is a multi-sectoral undertaking to be spearheaded by the Department of Environment and Natural Resources (DENR).

A

Implementation of the Act

113
Q
A

Chemistry for Engineers (4 decks)

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