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My Packs: (UWO) (CHEM 1302) > Chapter 1: 1.2 The Ideal Gas Law > Flashcards

Chapter 1: 1.2 The Ideal Gas Law Flashcards

1
Q

Avogadro’s law states that one mole of any ideal gas always…

A

Occupies the same volume at a given temperature and pressure, regardless of the gas in question

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2
Q

According to Avogadro’s Law, equal volumes of different gases at the same temperature and pressure…

A

Contains the same number of moles

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3
Q

Define:

Molar volume of a gas

A

Volume occupied by one mole of any gas

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4
Q

Define:

STP

Give units

A

Standard temperature and pressure

= 1 atm (101.324 kPa) and 273.15 K

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5
Q

Define and state the formula for:

Density

(in terms of gases)

A

Mass per unit volume
d = m/V

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6
Q

Show the relation and state the formula for:

Mass, molar mass, and moles

A

m = MM * n

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7
Q

What are the two forms of the ideal gas equation that can be used to derive relationship between gas density and its molar mass?

A

d = (MM)P / RT

OR

MM = dRT / P

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8
Q

State the relationships between gas density/molar mass at constant temperature

A

Gas density is directly proportional to its pressure

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9
Q

State the relationships between gas density/molar mass at constant temperature AND pressure

A

Density is related to molar mass of the gas

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10
Q

Define and state the formula for:

Dalton’s Law of Partial Pressures

A

A mixture of gases behaves as a single gas
PV = nRT or P(total) * V(total) = n(total) * R * T

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11
Q

Define:

Dalton’s Law of Partial Pressures

A

The total pressure exerted by a mixture of gases is the sum of all the partial pressures of these gases

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12
Q

State the formula for:

Mole fraction of any one gas in a mixture

A

X(i) = n(i)/n(T)
[mole fraction = # of moles of individual constituent / # of total moles in mixture]

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13
Q

State the proportionality in:

Mole Fractions

State constants

A

Pressure (P) is directly proportional to moles (n)

At constant temperature (T) and volume (V)

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14
Q

What must the mole fraction (ratio) equal to?

A

Must equal to the pressure ratio

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15
Q

What does the sum of all mole fractions equal?

A

1

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16
Q

At constant temperature and pressure, what is the relation between volume and moles?

A

Directly proportional

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17
Q

Define:

Vapour pressure

A

The partial pressure of water vapour

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18
Q

What does the vapour pressure of water depend on?

A

Only depends on the temperature of the water

19
Q

Does higher temperature mean more or less vapour pressure?

A

More

20
Q

Define:

Boiling point

A

Temperature at which the vapour pressure equals the atmospheric pressure

(Explains why water boils at lower temperatures at higher altitudes)

21
Q

True or False:

Solvents that are more volatile (have lower boiling points) have lower vapour pressures

A

False, solvents that are more volatile have higher vapour pressures

22
Q

Define:

Average Molar Mass of a mixture of different gases

A

The weighted average of the molar masses of the different components

23
Q

State the formula for:

Average molar mass of a gas mixture

A

MM (with a line above to represent weighted average) = XaMMa + XbMMb + XcMMc …

24
Q

State the assumptions of:

Kinetic Molecular Theory of Gases

A
  1. Size of particles is negligible
  2. Molecules are point particles (only Ek)
  3. Elastic collisions
  4. No intermolecular forces
  5. Kinetic energy (Ek) is proportional to temperature (Ek [line above] = 1/2mu^2 [u has line])
25
Q

What do bars/lines above values mean?

A

Average values

26
Q

What does the term u[bar]^2 mean? How is it found?

A

Mean-square speed
Found by taking an average of the squares of the speeds of the molecules

27
Q

What are the factors that determine the pressure of a gas in a container?

A
  1. Mass of each molecule (m)
  2. Speed of the molecules (u)
  3. Frequency of collisions/the number of collisions per second
28
Q

What does the frequency of collision relate to?

A
  1. The number of molecules (N)
  2. The volume of the container (V)
  3. The speed of the molecules (u)
29
Q

State:

The basic equation of the kinetic theory of gases

A

P = 1/3 (N/V)(mu[bar]^2)

30
Q

State the proportionalities of:

Mean-square speed of gas molecules, temperature, molar mass

A

Directly proportional to the temperature
Inversely proportional to the molar mass

31
Q

True or False:

If a gas is heated the molecules will move faster

A

True

32
Q

True or False:

If two gases are at the same temperature, the lighter gas molecules move slower, on average, then the heavier gas molecules

A

False, the lighter gas molecules move faster, on average, than the heavier gas molecules

33
Q

What does the Maxwell-Boltzmann distribution govern?

A

The distribution of the speeds of the molecules

34
Q

State the term and formula for:

The more commonly used form of the mean-square speed term

A

Root-mean-square (rms) speed
(sqrt)(3RT/MM)

35
Q

State the proportionality between:

rms speed and square root ratio of molar masses

A

The rms speed for the two gases is inversely proportional to the square root of the ratio of their molar masses

36
Q

What are the units for rms speed? In this scenario, state the units for molar mass and R

A

rms speed: metres per second
Molar mass: kilograms
R: 8.314 J/mol K OR 8.314 kg m^2/s^2 mol K

37
Q

Define:

Effusion

A

The flow of gas molecules at low pressures through tiny pores or pinholes in a container

38
Q

What is the rate of effusion defined as?

A

Number of moles of the gas escaping the container per unit of time

39
Q

State:

Graham’s Law

A

The rate of effusion of a gas is inversely proportional to the square root of its molar mass

40
Q

State the proportionality of:

Rate of effusion, Molar Mass

A

Rate of effusion is inversely proportional to the square root of its molar mass

r(effusion) proportional to 1/(sqrt)MM

41
Q

How is Graham’s Law written when two gases A and B with equal partial pressure effuse through a porous material or a small hole?

A

r(A)/r(B) = (sqrt)[ MM(B) / MM(A) ]

42
Q

True or False:

Lighter molecules effuse faster than heavier molecules

A

True

43
Q

What is the special about the gas that emerges from the container in effusion?

A

It is enriched in the lighter component

44
Q

What does the quantity f = (sqrt) [MM(B) / MM(A)] called?

A

Enrichment factor (how much of one gas is part of the effusion)

My Packs: (UWO) (CHEM 1302) (15 decks)

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