Gases Flashcards

1
Q

Gas molecules have very weak __ __, allowing gases to both ___ and change ___ to fill and take the shape of their containers.

A

intermolecular forces, flow, volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

An ideal gas is a hypothetical gas whose molecules have no __ ___ and occupy no ___. Under conditions of low ___ and high ____, many gases behave in nearly ideal fashion

A

intermolecular forces, volume, pressure, temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

The law that says a given gaseous sample at isothermal conditions will have a constant product of pressure and volume

A

boyle’s law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

States that at constant pressure, the quotient of the volume and temperature of gas is constant

A

charles law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Law that says for all gases at a constant temperature and pressure the volume of the gas will be directly proportional to the number of moles of gas present.

A

avogadro’s principle

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

One mole of an ideal gas under STP conditions has a volume of _____ L

A

22.4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

As the pressure of a gas increases, the particles are pushed closer together, and the ___ ___ for a given temperature is approached. This makes the ___ _____ ____ become more and more significant until the gas condenses into a liquid state. At moderately high pressure, the volume of a gas is ___ than would be predicted by the ideal gas law.

A

condensation pressure, intermolecular attraction forces, larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

As the temperature of a gas is decreased, the ___ ___ of the gas molecules decreases and the attractive intermolecular forces become significant. As the ____ ____ is approached for a given pressure, intermolecular attractions eventually cause the gas to _____ into a liquid state, and the attractions cause the gas to have a ___ volume than would be predicted by the ideal gas law. The closer the temperature of a gas is to its ___ ___, the less ideal is its behavior

A

average velocity, condensation temperature, condense, smaller, boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

the pressure exerted by each individual gas

A

partial pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

states that the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components

A

dalton’s law of partial pressures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Assumptions of the kinetic molecular theory are that gases are made up of particles whose volumes are ____ compared to the container volume, the gas atoms or molecules are ____ and and exhibit no ___ ___ or ___, gas particles are in ___ __ motion, undergoing collisions with other particles and the container walls, collisions between any two gas particles are ____, meaning there is no overall gain or loss of energy, and the average kinetic energy of gas particles is proportional to the ___ ___ of the gas and is the same for the gas and is the same for all gases at a given temperature

A

negligible, inert, intermolecular attraction, repulsion, continuous, random, elastic, absolute temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

The _____ __ ___ shows the distribution of speeds of gas particles at a given temperature. The ___ ___ of all gas particles can be related to the temperature, but the speed of an individual molecules is impossible to define

A

maxwell-boltzmann distribution, average soeed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

____ of gases can provide a demonstration of random motion when the molecules of these gases mix with one another by virtue of their individual __ ___. Diffusion occurs when gas molecules move through a ____. The kinetic molecular theory of gases predicts that ____ gas molecules diffuse more slowly than ___ ones because of their differing ___ _____.

A

diffusion, kinetic properties, mixture, heavier, lighter, average speeds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Under isothermal and isobaric conditions, the rates at which two gasses diffuse are inversely proportional to the ___ __ of their ___ ___.

A

square root, molar masses

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

___ is the flow of gas particles under pressure from one compartment to another through a __ ____. For two gases at the same ___, the rates of effusion are proportional to the __ ___. They also have the same relationship to __ __ as that for diffusion

A

effusion, small opening, temperature, average speeds, molar mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly