Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry for Today > Chapter 5 - Gases > Flashcards

Chapter 5 - Gases Flashcards

(53 cards)

Start Studying
1
Q

_______ is the force exerted per unit area by gas molecules as they strike the surfaces around them.

A

Pressure

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

The pressure that a gas sample exerts is the _____ that results from the collisions of gas particles divided by the ____ of the surface with which they collide.

A

force, area

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

Pressure =

A

force/area

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

mmHg originates from how pressure is measured with a _______.

A

barometer

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

A _______ is an evacuated glass tube, the tip of which is submerged in a pool of mercury.

A

barometer

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

In a barometer, when the atmospheric pressure _____, the height of the mercury column _____ as well. Similarly, when the atmospheric pressure _____, the height of the column _____.

A

rises, rises. falls, falls.

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

The unit millimeter of mercury is often called a ____.

A

torr

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

1 mmHg = __ torr

A

1

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

A second unit of pressure is the __________ (___), the average pressure at sea level.

A

atmosphere, (atm)

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

1 atm = ___ mmHg

A

760

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

The SI unit of pressure is the ______ (__).

A

pascal (Pa)

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

We can measure the pressure of a gas sample in the laboratory with a _________. A _________ is a U-shaped tube containing a dense liquid, usually mercury.

A

manometer

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

What are the four basic properties of a gas sample?

A

Pressure (P), volume (V), temperature (T) and amount in moles (n).

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

Boyle’s law says…

A

Volume is inversely proportional to pressure.

V ∞ 1/P, constant T,n

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

According to Boyle’s law, if the volume of a gas sample is decreased, the same number of gas particles is crowed into a smaller volume, resulting in more collisions with the walls and therefore an ______ in the pressure.

A

increase.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the equation for Boyle’s law?

A

P1V1=P2V2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Charles’s law says…

A

Volume is directly proportional to temperature.

V ∞ T, constant P,n

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

According to Charles’s law, the volume of a gas increases with _________ temperature.

A

increasing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the equation for Charles’s law?

A

V1/T1=V2/T2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Avogadro’s law says…

A

Volume is directly proportional to the number of gas molecules (moles)
V ∞ n, constant P, T

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

According to Avogadro’s law, when the amount of gas in a sample increases at constant temperature and pressure, its volume _______ in direct proportion because the greater number of gas particles fill more space.

A

increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the equation for Avogadro’s law?

23
Q

What is the equation for the Ideal Gas law?

24
Q

What does R = ?

25
The volume occupied by one mole of a substance is its _____ ______
molar volume
26
Under STP conditions, T = ____ K, P = ____ atm, and V = ____ L
``` T = 273.15K P = 1.00atm V = 22.4L ```
27
Density =
molar mass/molar volume
28
The density of a gas is ______ proportional to its molar mass. The greater the molar mass of a gas, the ____ dense the gas.
directly, more
29
d =
(P)(MM)/(R)(T)
30
1 atm = ____ psi
14.7
31
The pressure due to any individual component in a gas mixture is its _______ _______.
partial pressure
32
What is Dalton's law of partial pressures?
Ptotal = Pa + Pb + Pc + ...
33
How do you calculate Mole Fraction?
Xa = na/ntotal, or simply Pa=Xa(Ptotal)
34
Low oxygen levels produce a physiological condition called _______ or oxygen starvation.
hypoxia
35
When Po2 increases beyond 1.4 atom, the increased oxygen concentration in body tissues causes a condition called _______ _______, which results in muscle twitching, tunnel vision, and convulsions.
oxygen toxicity
36
When PN2 increases beyond about 4 atm, a condition called _______ ______ or "rapture of the deep" results.
nitrogen narcosis
37
The partial pressure of water in the mixture, called the _____ _______, depends on the temperature.
vapor pressure
38
Scientific laws summarize behavior - for example, Charles's law summarizes ___ the volume of a gas depends on temperature --- while theories give the underlying reason for the behavior. A theory of gas behavior explains, for example, ___ the volume of a gas increases with increasing temperature.
how, why
39
What are the three postulates of kinetic molecular theory?
1. The size of a particle is negligibly small. 2. The average kinetic energy of a particle is proportional to the temperature in kelvins. 3. The collision of one particle with another (or with the walls of its container) is completely elastic.
40
The ______ kinetic energy, NOT velocity, is proportional to temperature.
average
41
What is the equation for kinetic energy?
(1/2)mv^2
42
The atoms in a sample of helium and a sample of argon at the same temperature have the same average kinetic energy but not the same average _______.
velocity
43
Since the helium atoms are lighter, they must move faster to have the same ______ energy as argon atoms.
kinetic
44
The force (F) associated with an individual collision is given by F =
F = ma
45
What is the root mean square velocity equation?
urms √(3RT)/(MM)
46
The lighter the particle, the _____ it will move and the ______ the range will be.
faster, longer
47
The higher the temperature, the _____ the average velocity will be, and the ______ the range of velocity will be
higher
48
The average distance that a molecule travels between collisions is its _____ ____ ____
mean free path
49
Mean free path increases with _________ pressure.
decreasing
50
The process by which gas molecules spread out in response to a concentration gradient is ________.
diffusion
51
The process by which a gas escapes from a container into a vacuum through a small whole is _________.
effusion
52
What is the equation of Graham's law of effusion?
Rate A/Rate B = √(MM B)/(MM A)
53
1 mole = ____ L under STP conditions
22.4

Chemistry for Today (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions