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Chemistry 01 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Matter exists in what three distinct physical states?

A

Gas
Liquid
Solid

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2
Q

Name three properties of a gas.

A

1) Uniformly fills any container
2) Is easily compressed
Mixes completely with any other gas.

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3
Q

As a gas, water occupies ________ times as much space as it does as a liquid at 25C and atmospheric pressure.

A

12000

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4
Q

What is a barometer?

A

A device to measure atmospheric pressure.

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5
Q

Who invested the barometer?

A

Evangelista Torricelli in 1643

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6
Q

What are two common units used for pressure?

A

mm Hg - Height of the mercury column in millimeters, also call the torr

Standard atmosphere, atm

1 atm = 760 mm Hg = 760 torr

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7
Q

What is the equation for pressure?

A

Pressure = force / area

In SI system, force is measured in newton (N) and area in meters squared (m^2)

The unit of pressure in the SI system is newtons per meter squared (N/m^2) and is call the pascal (Pa)

1 standard atmosphere = 101,325 Pa

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8
Q

What is a Pascal?

A

The unit of pressure in the SI system is newtons per meter squared (N/m^2) and is call the pascal (Pa)

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9
Q

What did Robert Boyle do?

A

Performed the first quantitative experiments on gases.

Studies the relationships between the pressure of trapped gases and their volume.

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10
Q

What is Boyle’s law?

A

PV = k

P1V1 = P2V2

Where k is a constant for a given sample of air at a specific temperature.

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11
Q

What type of relationship exists between pressure and volume?

A

Inverse relationship.

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12
Q

Is Boyle’s law always accurate?

A

No, works better at low pressures.

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13
Q

What is an Idea Gas?

A

A gas that strictly obeys Boyle’s law.

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14
Q

Where does a gas act most ideally?

A

Close to zero pressure.

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15
Q

Explain Charles’s law.

A

Charles found in 1787 that the volume of a gas at constant pressure increases linearly with the temperature of the gas. That is, a plot of the volume of a gas (at constant pressure) versus its temperature C gives a straight line.

The volume of each gas is directly proportional to temperature and extrapolates to zero when the temperature is 0 K.

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16
Q

What is Kelvin?

A

A unit of temperature measurement

K = C + 273

The volumes of gases extrapolate to zero at the same temperature, -273 C or 0 K

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17
Q

What is Charles’s law?

A

V = bT

V1/T1 = V2/T2

Where T is in kelvins and b is a proportionality constant.

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18
Q

What is the importance of 0 K?

A

At temperatures below this point, the extrapolated volumes would become negative. The fact that a gas cannot have a negative volume suggests that 0 K has a special significance. In fact, 0 K is call absolute zero, there is much evidence to suggest that this temperture cannot be attained.

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19
Q

Explain Avogadro’s law?

A

Equal volumes of gases at the same temperature and pressure contain the same number of “particles”

For a gas a constant temperature and pressure, the volume is directly proportional to the number of moles of gas. This relationship is obeyed closely by gases at low pressures.

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20
Q

What is Avogadro’s law?

A

V = an

V1/n1 = V2/n2

V is volume
n is the number of moles of gas particles
a is a proportionality constant.

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21
Q

Explain the Ideal Gas Law

A

Consider Bolye’s, Charles’s, and Avogadro’s laws. These relationships, which show how the volume of gas depends on pressure, temperature, and the number of moles of gas present. These can be combined into one equation, the ideal gas law.

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22
Q

What is the Ideal Gas Law?

A

V = R * (Tn / P)

of

PV = nRT

where R is the combined proportionality constant called the universal gas constant.

R = 0.08206 (L atm) / (K mol)

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23
Q

A particular state of a gas is describe by …

Study These Flashcards
A

Pressure
Volume
Temperature
Number of Moles

24
Q

The real advantage of using the ideal gas law is that it applies to virtually any problem dealing with gases and is easy to remember.

25
True of False - Temperature must always to converted to the Kelvin scale.
True
26
Who is likely the best chemist that ever lived?
Kayla
27
What is molar volume?
22.42 L is the molar volume of an ideal gas (at 0 C and 1 atm)
28
What is standard temperature and pressure?
STP 0 C and 1 atm
29
What is Molar mass
Molar mass = (dRT) / P where d = density = mass / volume Density is in units grams per liter.
30
Which world famous chemist likely broke the most test tubes?
Christopher
31
Explain Dalton's law.
In 1803 Dalton summarized his observations as follows: For a mixture of gases in a container, the total pressure exerted is the sum of the pressures that each gas would exert if it were alone. This statement is known as Dalton's law of partial pressures.
32
What is Dalton's law?
P total = P1 + P2 + P3 + ... Or P total = P1 + P2 + ... = (n1RT)/V + (n2RT)/V + ... = (n1 + n2 + ...)(RT/V) = ntotal(RT/V) where ntotal is the sum of the number of moles of various gases.
33
The fact that the pressure exerted by an ideal gas is not affected by the identity (composition) of the gas particles reveals what two things about ideal gases?
1) the volume of the individual gas particle must not be important. 2) the forces among the particles must not be important.
34
Define mole fraction.
The ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture. x1 = n1 / n total x1 = P1 / P total
35
What is a law?
A law is a way of generalizing behavior that has been observed in many experiments. Laws are very useful, since they allow us to predict the behavior of similar systems. Although laws summarize observed behavior, they do not tell us why nature behaves in the observed fashion.
36
What is a model?
A model is considered successful if it explains the observed behavior in question and predicts correctly the results of future experiments. It is important to understand that a model can never be proved absolutely true. in fact, any model is an approximation by its very nature and is bound to fail at some point.
37
What are the Postulates of the Kinetic Molecular Theory?
1. The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be negligible (zero). 2. The particles are in constant motion. The collisions of particles with the walls of the container are the cause of pressure exerted by the gas. 3. The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other. 4. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas. The molecules in a real gas have finite volumes and do exert forces on each other. Thus real gases do not conform to these assumptions.
38
What is the real test of a model?
The true test of a model is how well its predictions fit the experimental observations.
39
What does the volume of a gas depend on?
The volume of a gas (at constant P and T) depends only on the number of gas particles present.
40
What is the average kinetic energy equation?
(KE) avg = 3/2 RT
41
Explain the root mean square velocity.
In the equation from the kinetic molecular theory, the average velocity of the gas particles is a special kind of average. The symbol u^2 bar means the average of the squares of the particle velocities. The square root of u^2 bar is call the root mean square velocity. u rms = (u^2)^1/2 u rms = sq root (3RT/M) where M = Na x m ``` m = the mass in kilograms of a single pas particle. Na = the number of particles in a mole ```
42
What is a Joule?
A joule is defined as a kilogram meter squared per second squared (kg * m^2/s^2) A joule is the energy unit most often used in the SI system.
43
True of False - If the path of a particular gas particles could be monitored, it would look very erratic.
True
44
What is mean free path?
The average distance a particles travels between collisions in a particular gas sample.
45
What is one effect of the many collisions among gas particles?
One effect of the many collisions among gas particles is to produce a large range of velocities as the particles collide and exchange kinetic energy.
46
What is the effect of temperature on the velocity distribution in a gas?
As the temperature is increased, the curve peak moves toward higher values and the range of velocities becomes much larger.
47
What is Difusion?
Diffusion is the term used to describe the mixing of gases.
48
What is Effusion?
Effusion is the term used to describe the passage of a gas through a tiny orifice into an evacuated chamber.
49
What is Graham's law of effusion?
(Rate of effusion for gas 1) / (Rate of effusion for gas 2) = square root M2 / square root of M1 Where M1 and M2 represents the molar masses of the gases.
50
Do ideal gases exist? Explain.
An ideal gas is hypothetical concept. No gas exactly follows the ideal gas law, although many gases come very close at low pressures and/or high temperatures. Thus ideal gas behavior can best be thought of as the behavior approached by real gases under certain conditions.
51
When do real gases typically exhibits behavior that is closest to ideal behavior.
At low pressures and high temperatures.
52
What does the van der Waals equation do?
Corrects for pressure and volume
53
What are the principle components of the atmosphere?
N2 and O2
54
What does the upper atmosphere do?
The upper atmosphere serves as an important shield to prevent high-energy radiation from reaching the earth.
55
What does Ozone do?
The Ozone in the upper atmosphere helps prevent high-energy ultraviolet radiation from penetrating to the earth.

Chemistry 01 (3 decks)

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