L1-L2 Flashcards

1
Q

A set of characteristically quantitative approaches to the study of chemical problems

A

physical chemistry

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2
Q

Thermodynamics explains ____ reactions occur (aka the ____ ___ of the reactions) and the ____ a reaction generates or requires

A

why, driving force, energy

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3
Q

Gases form the ___ ___ of many machines (e.g. heat engines and ____). The gas phase is the ____ state of matter to treat theoretically, and it shows ____ behaviour that is _____.

A

working substance, refrigerators, simplest, limiting, universal

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4
Q

The ___ of a system is defined by a particular set of properties such as ___, ___, and ___. These properties can be related by an algebraic expression called an equation of state, such as the ___ ___ ____

A

state, temperature, volume, moles, ideal gas law

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5
Q

Ideal gas assumes that the gas molecules do not occupy any ____, and there are no ____ between the gas molecules

A

volume, interactions

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6
Q

The ideal gas law can describe many gasses at high _____ and low ____

A

temperature, pressures

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7
Q

A molecular interpretation of the ideal gas law that leads to a relation between internal energy and temperature

A

kinetic model of gasses

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8
Q

Assumptions for the kinetic model of gasses are that a gas consists of molecules in _____ motion, gas molecules are _____ ____ points, the molecules move in ____ ____ until they collide, and the molecules do not ____ except during collisions

A

random, infinitesimally small, straight lines, interact

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9
Q

In the kinetic model of gasses, the pressure arises from the force exerted on the ____ of the container when the impacting molecules are _____. We need to know the ___ of each impact and the number of impacts in a given interval. We find that the average ___ ___ ___ of one mole of an ideal gas, in other words the ___ ___, is only dependent on ____

A

walls, deflected, force, translational kinetic energy, internal energy, temperature

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10
Q

The equipartition principle states that each translational and ____ degree of freedom contributes _____ to the total energy, and each vibrational degree of freedom contributes ______ to the total internal temperature.

A

rotational, RT/2, RT

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11
Q

Rigid, diatomic molecules have _______, because there are ___ translational, ___ vibrational, and ___ rotational degrees of freedom. However, at room temperature, the ___ ____ ___ is not reached for ______ energy, thus it is not ____. This makes the internal energy of one mole of diatomic molecule, to be ____ at room temperature

A

U = 7/2RT, 3, 1, 2, high temperature limit, vibrational, excited, U = 5/RT

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12
Q

A monoatomic molecule only has ___ degrees of ____ freedom

A

3, translational

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13
Q

In real gasses, the ____ ___ of the molecules and the ____ between them lead to deviations from the ideal gas law. Consequently, the internal energy is no longer a function of ____ alone.

A

finite size, interactions, temperature

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14
Q

The repulsive interaction between molecules (aka the ___ ___), implies that they cannot come closer than a certain ____. The actual volume in which the molecules can move is thus _____ compared with the volume of the container V. Therefore, replace V in the ideal gas law by _____, where b is the volume / ___ occupied by the gas itself

A

size effect, distance, reduced, V-nb, mole

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15
Q

The energy of ___ one molecule experiences from the other molecules is proportional to the density, n/V. The total energy of attraction is thus proportional to ____. These forces ___ the pressure that the gas exert, and since pressure is energy per volume, the resulting change in pressure is proportional to _______. Thus, the pressure in the ideal gas law is replaced by ______

A

attraction, (n n/V), reduce, (n^2/v^2), P + a(n^2/v^2)

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16
Q

The compressibility factor is _______. the value is __ for an ideal gas

A

z = pV/nRT, 1

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17
Q

The virial equation shows that at ____ pressures, one often observes a ___ ___ of z with pressure. This linear behaviour can be described by the first two terms in the general virial equation: ____

A

moderate, linear dependence, z = PV/nRT = 1 + B2p (P)

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18
Q

The. virial equation is a series _____ in terms of pressure or an ____ power of molar volume, Vm. The virial equation has the most sound ____ foundation and can achieve desirable accuracy

A

expansion, inverse, theoretical

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19
Q

The interface between the system and the surroundings

A

boundary

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20
Q

Can exchange both energy and matter with its surroundings

A

open system

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21
Q

Can exchange energy but not matter with its surroundings

A

closed system

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22
Q

can exchanged neither energy nor matter with its surroundings

A

isolated system

23
Q

a physical property that depends only on the present state of the system and is independent of how the state was prepared and the past history of the system

A

state function

24
Q

some examples of state functions

A

density, internal energy, pressure, volume, temperature

25
a constant temperature process. (it may be necessary for the surroundings to act as a heat reservoir or sink in order to keep the system temperature fixed, and that in general, the system boundary must permit heat flow)
isothermal process
26
(P = Psurr = constant) a constant pressure process
isobaric process
27
a constant volume process
isochoric process
28
a process in which no heat enters or leaves the system
adiabatic process
29
a process that releases heat into the surroundings (system loses energy)
exothermic process
30
a process that absorbs heat from the surroundings (the system gains energy)
endothermic process
31
In a reversible process, the system is always in _____. The process can be reversed by an ____ ___ of its properties. At the end of a cycle, both the system and surroundings have been returned to their ___ __ without any ___ change to either. Sometimes, this is referred to as a _____ process. The ____ of the process is not predetermined.
equilibrium, infinitesimal change, initial states, permanent, quasi-static, direction
32
In an irreversible system, the system is not always in ____. At the end of a cycle, the system has been returned to its initial state, but the ____ have not, and experienced a permanent change.
equilibrium, surroundings
33
Spontaneous processes have a predetermined ___ and are ____.
direction, irreversible
34
Defines the temperature 0C as 273.15 K
Zeroth law of thermodynamics
35
States that for an isolated system, the internal energy is constant, and equal to q + w (energy can neither be created or destroyed)
first law of thermodynamics
36
q and q are not ___ functions, they are path _____
state, dependent
37
Energy can be exchanged between a closed system through the transfer of ___ or ____
heat, work
38
an endothermic reaction has a _____ q, while an exothermic reaction has a ____ q
positive, negative
39
Heat was first thought to be a fluid called ___, which flows from a hot substance to a cooler one. ____ suggested that is a form of energy. He found that he could raise the temperature of a substance by either ___ it or by ___ ___ it
caloric, joule, heating, vigorously stirring
40
If the surroundings do work on the system, w is _____, and the system gains energy. If the system does work on the surroundings, w is ____ and the system loses energy
positive, negative
41
Only under ____ (e.g. equilibrium) conditions, does the external pressure equal the pressure of the ____
reversible, system
42
When a gas expands reversibly, the ____ pressure is matched to the pressure of the ____ at every stage of the expansion. When the steps corresponding to the increase in volume are ______, maximum ___ is done on the _____, while the ____ amount of work is required from the surroundings.
external, gas, infinitesimal, work, surroundings, minimum
43
The internal energy of an ideal gas ____ __ ___ in an isothermal process, and thus, ____
does not change, q= -w
44
the measurement of heat
calorimetry
45
the heat absorbed by an object dividing by the corresponding temperature change
heat capacity
46
The heat capacity generally depends on whether the ___ or the ____ is kept constant. In general, the heat capacity is not a ____ function because it is path-dependent.
pressure, volume, state
47
___, ___ and ____ have low heat capacities, while water, ___ and ____ have high heat capacities
brass, copper, stainless steel, liquid, ethanol
48
Enthalpy is defined as ____ and helps keep track of heat exchange at constant ____.
H = U + PV, pressure
49
A chemical reaction almost always involves changes in ____.
Heat
50
the standard enthalpy for its formation from its element in their standard state at a given temperature and pressure
standard enthalpy of formation
50
the standard enthalpy of formation of an ____ is equal to ___ by definition
element, 0
51
the pure form of a substance at 1 atm
standard sate of a substance
52
For a reversible phase transition at constant T and P, change in gibbs free energy equals ___ and ____
0, H = TS